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6 Apr 2023
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Aasiyah Rahman
@aasiyahrahman
A buffer solution helps maintain a stable pH when small... Show more
A buffer solution's pH calculation requires careful consideration of acid dissociation constants and equilibrium principles. When working with weak acids like HX, understanding how to calculate pH of buffer solution at 298K involves applying mathematical relationships between concentration and dissociation constants.
Definition: A buffer solution is a mixture of a weak acid and its salt that maintains a relatively constant pH when small amounts of acid or base are added.
The calculation process involves using the acid dissociation constant and the Henderson-Hasselbalch equation. For a weak acid HX with Ka = 3.01 × 10⁻⁵ mol/dm³, we must consider both the initial concentrations and the equilibrium established in the solution.
When solving buffer problems, it's essential to recognize that temperature affects the equilibrium constant and, consequently, the pH. At 298K , these calculations become standardized, making it a common reference temperature for buffer calculations.
Understanding water's ionic product is fundamental to pH calculations at various temperatures. The relationship between temperature and Kw directly impacts the pH of pure water and solutions.
Vocabulary: Kw represents the product of H+ and OH- ion concentrations in water at a specific temperature.
At elevated temperatures like 42°C, Kw changes from its standard value, affecting the pH of pure water. Similarly, when working with solutions like sodium hydroxide at 75°C, the changed Kw value influences the overall pH calculations.
The temperature dependence of Kw demonstrates how pH values can vary significantly under different conditions, even in pure water systems.
Understanding the methanoic acid dissociation constant expression is crucial for calculating solution pH. Methanoic acid undergoes partial dissociation in water, establishing an equilibrium that determines the solution's acidity.
Example: The dissociation equation: HCOOH ⇌ H+ + HCOO- The Ka expression: Ka = /
With a Ka value of 1.78 × 10⁻⁴ mol/dm³ at 25°C, calculating the pH of methanoic acid solutions requires considering both the initial concentration and the extent of dissociation. The endothermic nature of the dissociation process affects how temperature changes influence the solution's pH.
Understanding how to calculate pH after adding hydrochloric acid to buffer solution requires knowledge of buffer capacity and equilibrium principles. When working with methanoic acid and sodium methanoate buffers, the ratio of acid to salt determines the buffer's pH.
Highlight: Buffer capacity depends on both the total concentration of the buffer components and their ratio.
For a buffer containing specific concentrations of methanoic acid and sodium methanoate, the pH calculation involves using the Henderson-Hasselbalch equation while considering the system's temperature and Ka value. The buffer's resistance to pH change comes from its ability to neutralize added acids or bases through shifting equilibrium positions.
The practical applications of such calculations extend to biological systems, where maintaining constant pH is crucial for proper cellular function.
A buffer solution maintains a relatively constant pH when small amounts of acid or base are added. Let's explore how to calculate pH of buffer solution at 298K and understand the effects of adding acids.
When hydrochloric acid is added to a buffer solution, it's crucial to consider how this strong acid affects the equilibrium. The added H+ ions from HCl will react with the basic component of the buffer, shifting the equilibrium according to Le Chatelier's principle. This interaction helps maintain the buffer's pH within a narrow range, though some change will occur.
To calculate the new pH after adding HCl, we need to:
Definition: A buffer solution contains a weak acid and its salt that resist changes in pH when small amounts of acid or base are added.
Understanding Brønsted-Lowry acids is fundamental to chemistry. A Brønsted-Lowry acid is a proton donor, and this concept helps explain acid-base reactions at the molecular level.
The methanoic acid dissociation constant expression represents the extent to which an acid dissociates in water. For ethanoic acid, the Ka expression is: Ka = /
When dealing with chloroethanoic acid , its higher Ka value indicates it's a stronger acid than ethanoic acid. This increased acidity is due to the electron-withdrawing effect of the chlorine atom, which stabilizes the conjugate base.
Example: For ethanoic acid with Ka = 1.75 × 10-5 mol/dm3, a pH of 2.69 indicates significant dissociation in the solution.
The selection of appropriate indicators for acid-base titrations depends on the strength of both the acid and base involved. The indicator's pH range must overlap with the pH at the equivalence point for accurate results.
For strong acid-strong base titrations, both methyl orange and phenolphthalein can work effectively. However, for weak acid-weak base titrations, indicator selection becomes more critical due to the buffer region near the equivalence point.
Highlight: The equivalence point pH varies depending on the relative strengths of the acid and base. Strong acid-strong base titrations have an equivalence point at pH 7, while other combinations differ.
Carboxylic acids exemplify weak acids in organic chemistry. Their partial dissociation in water creates equilibrium between the acid and its ions. To calculate pH after adding hydrochloric acid to buffer solution, we must consider both the initial equilibrium and the effect of the added strong acid.
When working with weak acids like propanoic acid, their reactions with bases like sodium carbonate produce salt and carbonic acid, which decomposes to water and carbon dioxide. Understanding these reactions is crucial for laboratory work and industrial applications.
Vocabulary: The term "weak" when applied to acids means they partially dissociate in aqueous solutions, establishing an equilibrium between the acid and its ions.
The acid dissociation constant is fundamental to understanding how acids behave in solution. When working with benzenecarboxylic acid , we need to understand both its dissociation behavior and how to calculate pH of buffer solution at 298K.
The methanoic acid dissociation constant expression for benzenecarboxylic acid can be written as: Ka = / where the square brackets represent the molar concentrations of each species at equilibrium. This expression shows how the acid breaks apart in water to form hydrogen ions and the conjugate base.
Definition: The acid dissociation constant measures the extent to which an acid dissociates in water, with larger values indicating stronger acids.
When calculating the pH of a 0.0120 mol/dm³ benzenecarboxylic acid solution, we follow these detailed steps:
Example: For a 0.0120 mol/dm³ solution:
Understanding how buffer solutions maintain pH when acids or bases are added is crucial in chemistry. When calculating pH after adding hydrochloric acid to buffer solution, we must consider the buffer's capacity and initial concentrations.
Buffer solutions resist pH changes through the equilibrium between the weak acid and its conjugate base. The Henderson-Hasselbalch equation helps us understand this relationship: pH = pKa + log
Highlight: Buffer capacity depends on:
When adding strong acids like HCl to a buffer, the conjugate base neutralizes the added H⁺ ions, minimizing pH changes. This process demonstrates the practical importance of buffers in maintaining stable pH conditions in various applications, from biological systems to industrial processes.
Vocabulary: Buffer capacity refers to the amount of acid or base a buffer can neutralize before significant pH changes occur.
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The app is very easy to use and well designed. I have found everything I was looking for so far and have been able to learn a lot from the presentations! I will definitely use the app for a class assignment! And of course it also helps a lot as an inspiration.
Stefan S
iOS user
This app is really great. There are so many study notes and help [...]. My problem subject is French, for example, and the app has so many options for help. Thanks to this app, I have improved my French. I would recommend it to anyone.
Samantha Klich
Android user
Wow, I am really amazed. I just tried the app because I've seen it advertised many times and was absolutely stunned. This app is THE HELP you want for school and above all, it offers so many things, such as workouts and fact sheets, which have been VERY helpful to me personally.
Anna
iOS user
Best app on earth! no words because it’s too good
Thomas R
iOS user
Just amazing. Let's me revise 10x better, this app is a quick 10/10. I highly recommend it to anyone. I can watch and search for notes. I can save them in the subject folder. I can revise it any time when I come back. If you haven't tried this app, you're really missing out.
Basil
Android user
This app has made me feel so much more confident in my exam prep, not only through boosting my own self confidence through the features that allow you to connect with others and feel less alone, but also through the way the app itself is centred around making you feel better. It is easy to navigate, fun to use, and helpful to anyone struggling in absolutely any way.
David K
iOS user
The app's just great! All I have to do is enter the topic in the search bar and I get the response real fast. I don't have to watch 10 YouTube videos to understand something, so I'm saving my time. Highly recommended!
Sudenaz Ocak
Android user
In school I was really bad at maths but thanks to the app, I am doing better now. I am so grateful that you made the app.
Greenlight Bonnie
Android user
very reliable app to help and grow your ideas of Maths, English and other related topics in your works. please use this app if your struggling in areas, this app is key for that. wish I'd of done a review before. and it's also free so don't worry about that.
Rohan U
Android user
I know a lot of apps use fake accounts to boost their reviews but this app deserves it all. Originally I was getting 4 in my English exams and this time I got a grade 7. I didn’t even know about this app three days until the exam and it has helped A LOT. Please actually trust me and use it as I’m sure you too will see developments.
Xander S
iOS user
THE QUIZES AND FLASHCARDS ARE SO USEFUL AND I LOVE THE SCHOOLGPT. IT ALSO IS LITREALLY LIKE CHATGPT BUT SMARTER!! HELPED ME WITH MY MASCARA PROBLEMS TOO!! AS WELL AS MY REAL SUBJECTS ! DUHHH 😍😁😲🤑💗✨🎀😮
Elisha
iOS user
This apps acc the goat. I find revision so boring but this app makes it so easy to organize it all and then you can ask the freeeee ai to test yourself so good and you can easily upload your own stuff. highly recommend as someone taking mocks now
Paul T
iOS user
The app is very easy to use and well designed. I have found everything I was looking for so far and have been able to learn a lot from the presentations! I will definitely use the app for a class assignment! And of course it also helps a lot as an inspiration.
Stefan S
iOS user
This app is really great. There are so many study notes and help [...]. My problem subject is French, for example, and the app has so many options for help. Thanks to this app, I have improved my French. I would recommend it to anyone.
Samantha Klich
Android user
Wow, I am really amazed. I just tried the app because I've seen it advertised many times and was absolutely stunned. This app is THE HELP you want for school and above all, it offers so many things, such as workouts and fact sheets, which have been VERY helpful to me personally.
Anna
iOS user
Best app on earth! no words because it’s too good
Thomas R
iOS user
Just amazing. Let's me revise 10x better, this app is a quick 10/10. I highly recommend it to anyone. I can watch and search for notes. I can save them in the subject folder. I can revise it any time when I come back. If you haven't tried this app, you're really missing out.
Basil
Android user
This app has made me feel so much more confident in my exam prep, not only through boosting my own self confidence through the features that allow you to connect with others and feel less alone, but also through the way the app itself is centred around making you feel better. It is easy to navigate, fun to use, and helpful to anyone struggling in absolutely any way.
David K
iOS user
The app's just great! All I have to do is enter the topic in the search bar and I get the response real fast. I don't have to watch 10 YouTube videos to understand something, so I'm saving my time. Highly recommended!
Sudenaz Ocak
Android user
In school I was really bad at maths but thanks to the app, I am doing better now. I am so grateful that you made the app.
Greenlight Bonnie
Android user
very reliable app to help and grow your ideas of Maths, English and other related topics in your works. please use this app if your struggling in areas, this app is key for that. wish I'd of done a review before. and it's also free so don't worry about that.
Rohan U
Android user
I know a lot of apps use fake accounts to boost their reviews but this app deserves it all. Originally I was getting 4 in my English exams and this time I got a grade 7. I didn’t even know about this app three days until the exam and it has helped A LOT. Please actually trust me and use it as I’m sure you too will see developments.
Xander S
iOS user
THE QUIZES AND FLASHCARDS ARE SO USEFUL AND I LOVE THE SCHOOLGPT. IT ALSO IS LITREALLY LIKE CHATGPT BUT SMARTER!! HELPED ME WITH MY MASCARA PROBLEMS TOO!! AS WELL AS MY REAL SUBJECTS ! DUHHH 😍😁😲🤑💗✨🎀😮
Elisha
iOS user
This apps acc the goat. I find revision so boring but this app makes it so easy to organize it all and then you can ask the freeeee ai to test yourself so good and you can easily upload your own stuff. highly recommend as someone taking mocks now
Paul T
iOS user
Aasiyah Rahman
@aasiyahrahman
A buffer solution helps maintain a stable pH when small amounts of acid or base are added to the system.
The process to calculate pH of buffer solution at 298Krequires understanding several key components. First, you need to know... Show more
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A buffer solution's pH calculation requires careful consideration of acid dissociation constants and equilibrium principles. When working with weak acids like HX, understanding how to calculate pH of buffer solution at 298K involves applying mathematical relationships between concentration and dissociation constants.
Definition: A buffer solution is a mixture of a weak acid and its salt that maintains a relatively constant pH when small amounts of acid or base are added.
The calculation process involves using the acid dissociation constant and the Henderson-Hasselbalch equation. For a weak acid HX with Ka = 3.01 × 10⁻⁵ mol/dm³, we must consider both the initial concentrations and the equilibrium established in the solution.
When solving buffer problems, it's essential to recognize that temperature affects the equilibrium constant and, consequently, the pH. At 298K , these calculations become standardized, making it a common reference temperature for buffer calculations.
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Improve your grades
Join milions of students
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Understanding water's ionic product is fundamental to pH calculations at various temperatures. The relationship between temperature and Kw directly impacts the pH of pure water and solutions.
Vocabulary: Kw represents the product of H+ and OH- ion concentrations in water at a specific temperature.
At elevated temperatures like 42°C, Kw changes from its standard value, affecting the pH of pure water. Similarly, when working with solutions like sodium hydroxide at 75°C, the changed Kw value influences the overall pH calculations.
The temperature dependence of Kw demonstrates how pH values can vary significantly under different conditions, even in pure water systems.
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Improve your grades
Join milions of students
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Understanding the methanoic acid dissociation constant expression is crucial for calculating solution pH. Methanoic acid undergoes partial dissociation in water, establishing an equilibrium that determines the solution's acidity.
Example: The dissociation equation: HCOOH ⇌ H+ + HCOO- The Ka expression: Ka = /
With a Ka value of 1.78 × 10⁻⁴ mol/dm³ at 25°C, calculating the pH of methanoic acid solutions requires considering both the initial concentration and the extent of dissociation. The endothermic nature of the dissociation process affects how temperature changes influence the solution's pH.
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Understanding how to calculate pH after adding hydrochloric acid to buffer solution requires knowledge of buffer capacity and equilibrium principles. When working with methanoic acid and sodium methanoate buffers, the ratio of acid to salt determines the buffer's pH.
Highlight: Buffer capacity depends on both the total concentration of the buffer components and their ratio.
For a buffer containing specific concentrations of methanoic acid and sodium methanoate, the pH calculation involves using the Henderson-Hasselbalch equation while considering the system's temperature and Ka value. The buffer's resistance to pH change comes from its ability to neutralize added acids or bases through shifting equilibrium positions.
The practical applications of such calculations extend to biological systems, where maintaining constant pH is crucial for proper cellular function.
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A buffer solution maintains a relatively constant pH when small amounts of acid or base are added. Let's explore how to calculate pH of buffer solution at 298K and understand the effects of adding acids.
When hydrochloric acid is added to a buffer solution, it's crucial to consider how this strong acid affects the equilibrium. The added H+ ions from HCl will react with the basic component of the buffer, shifting the equilibrium according to Le Chatelier's principle. This interaction helps maintain the buffer's pH within a narrow range, though some change will occur.
To calculate the new pH after adding HCl, we need to:
Definition: A buffer solution contains a weak acid and its salt that resist changes in pH when small amounts of acid or base are added.
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Understanding Brønsted-Lowry acids is fundamental to chemistry. A Brønsted-Lowry acid is a proton donor, and this concept helps explain acid-base reactions at the molecular level.
The methanoic acid dissociation constant expression represents the extent to which an acid dissociates in water. For ethanoic acid, the Ka expression is: Ka = /
When dealing with chloroethanoic acid , its higher Ka value indicates it's a stronger acid than ethanoic acid. This increased acidity is due to the electron-withdrawing effect of the chlorine atom, which stabilizes the conjugate base.
Example: For ethanoic acid with Ka = 1.75 × 10-5 mol/dm3, a pH of 2.69 indicates significant dissociation in the solution.
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The selection of appropriate indicators for acid-base titrations depends on the strength of both the acid and base involved. The indicator's pH range must overlap with the pH at the equivalence point for accurate results.
For strong acid-strong base titrations, both methyl orange and phenolphthalein can work effectively. However, for weak acid-weak base titrations, indicator selection becomes more critical due to the buffer region near the equivalence point.
Highlight: The equivalence point pH varies depending on the relative strengths of the acid and base. Strong acid-strong base titrations have an equivalence point at pH 7, while other combinations differ.
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Carboxylic acids exemplify weak acids in organic chemistry. Their partial dissociation in water creates equilibrium between the acid and its ions. To calculate pH after adding hydrochloric acid to buffer solution, we must consider both the initial equilibrium and the effect of the added strong acid.
When working with weak acids like propanoic acid, their reactions with bases like sodium carbonate produce salt and carbonic acid, which decomposes to water and carbon dioxide. Understanding these reactions is crucial for laboratory work and industrial applications.
Vocabulary: The term "weak" when applied to acids means they partially dissociate in aqueous solutions, establishing an equilibrium between the acid and its ions.
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The acid dissociation constant is fundamental to understanding how acids behave in solution. When working with benzenecarboxylic acid , we need to understand both its dissociation behavior and how to calculate pH of buffer solution at 298K.
The methanoic acid dissociation constant expression for benzenecarboxylic acid can be written as: Ka = / where the square brackets represent the molar concentrations of each species at equilibrium. This expression shows how the acid breaks apart in water to form hydrogen ions and the conjugate base.
Definition: The acid dissociation constant measures the extent to which an acid dissociates in water, with larger values indicating stronger acids.
When calculating the pH of a 0.0120 mol/dm³ benzenecarboxylic acid solution, we follow these detailed steps:
Example: For a 0.0120 mol/dm³ solution:
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Understanding how buffer solutions maintain pH when acids or bases are added is crucial in chemistry. When calculating pH after adding hydrochloric acid to buffer solution, we must consider the buffer's capacity and initial concentrations.
Buffer solutions resist pH changes through the equilibrium between the weak acid and its conjugate base. The Henderson-Hasselbalch equation helps us understand this relationship: pH = pKa + log
Highlight: Buffer capacity depends on:
When adding strong acids like HCl to a buffer, the conjugate base neutralizes the added H⁺ ions, minimizing pH changes. This process demonstrates the practical importance of buffers in maintaining stable pH conditions in various applications, from biological systems to industrial processes.
Vocabulary: Buffer capacity refers to the amount of acid or base a buffer can neutralize before significant pH changes occur.
App Store
Google Play
The app is very easy to use and well designed. I have found everything I was looking for so far and have been able to learn a lot from the presentations! I will definitely use the app for a class assignment! And of course it also helps a lot as an inspiration.
Stefan S
iOS user
This app is really great. There are so many study notes and help [...]. My problem subject is French, for example, and the app has so many options for help. Thanks to this app, I have improved my French. I would recommend it to anyone.
Samantha Klich
Android user
Wow, I am really amazed. I just tried the app because I've seen it advertised many times and was absolutely stunned. This app is THE HELP you want for school and above all, it offers so many things, such as workouts and fact sheets, which have been VERY helpful to me personally.
Anna
iOS user
Best app on earth! no words because it’s too good
Thomas R
iOS user
Just amazing. Let's me revise 10x better, this app is a quick 10/10. I highly recommend it to anyone. I can watch and search for notes. I can save them in the subject folder. I can revise it any time when I come back. If you haven't tried this app, you're really missing out.
Basil
Android user
This app has made me feel so much more confident in my exam prep, not only through boosting my own self confidence through the features that allow you to connect with others and feel less alone, but also through the way the app itself is centred around making you feel better. It is easy to navigate, fun to use, and helpful to anyone struggling in absolutely any way.
David K
iOS user
The app's just great! All I have to do is enter the topic in the search bar and I get the response real fast. I don't have to watch 10 YouTube videos to understand something, so I'm saving my time. Highly recommended!
Sudenaz Ocak
Android user
In school I was really bad at maths but thanks to the app, I am doing better now. I am so grateful that you made the app.
Greenlight Bonnie
Android user
very reliable app to help and grow your ideas of Maths, English and other related topics in your works. please use this app if your struggling in areas, this app is key for that. wish I'd of done a review before. and it's also free so don't worry about that.
Rohan U
Android user
I know a lot of apps use fake accounts to boost their reviews but this app deserves it all. Originally I was getting 4 in my English exams and this time I got a grade 7. I didn’t even know about this app three days until the exam and it has helped A LOT. Please actually trust me and use it as I’m sure you too will see developments.
Xander S
iOS user
THE QUIZES AND FLASHCARDS ARE SO USEFUL AND I LOVE THE SCHOOLGPT. IT ALSO IS LITREALLY LIKE CHATGPT BUT SMARTER!! HELPED ME WITH MY MASCARA PROBLEMS TOO!! AS WELL AS MY REAL SUBJECTS ! DUHHH 😍😁😲🤑💗✨🎀😮
Elisha
iOS user
This apps acc the goat. I find revision so boring but this app makes it so easy to organize it all and then you can ask the freeeee ai to test yourself so good and you can easily upload your own stuff. highly recommend as someone taking mocks now
Paul T
iOS user
The app is very easy to use and well designed. I have found everything I was looking for so far and have been able to learn a lot from the presentations! I will definitely use the app for a class assignment! And of course it also helps a lot as an inspiration.
Stefan S
iOS user
This app is really great. There are so many study notes and help [...]. My problem subject is French, for example, and the app has so many options for help. Thanks to this app, I have improved my French. I would recommend it to anyone.
Samantha Klich
Android user
Wow, I am really amazed. I just tried the app because I've seen it advertised many times and was absolutely stunned. This app is THE HELP you want for school and above all, it offers so many things, such as workouts and fact sheets, which have been VERY helpful to me personally.
Anna
iOS user
Best app on earth! no words because it’s too good
Thomas R
iOS user
Just amazing. Let's me revise 10x better, this app is a quick 10/10. I highly recommend it to anyone. I can watch and search for notes. I can save them in the subject folder. I can revise it any time when I come back. If you haven't tried this app, you're really missing out.
Basil
Android user
This app has made me feel so much more confident in my exam prep, not only through boosting my own self confidence through the features that allow you to connect with others and feel less alone, but also through the way the app itself is centred around making you feel better. It is easy to navigate, fun to use, and helpful to anyone struggling in absolutely any way.
David K
iOS user
The app's just great! All I have to do is enter the topic in the search bar and I get the response real fast. I don't have to watch 10 YouTube videos to understand something, so I'm saving my time. Highly recommended!
Sudenaz Ocak
Android user
In school I was really bad at maths but thanks to the app, I am doing better now. I am so grateful that you made the app.
Greenlight Bonnie
Android user
very reliable app to help and grow your ideas of Maths, English and other related topics in your works. please use this app if your struggling in areas, this app is key for that. wish I'd of done a review before. and it's also free so don't worry about that.
Rohan U
Android user
I know a lot of apps use fake accounts to boost their reviews but this app deserves it all. Originally I was getting 4 in my English exams and this time I got a grade 7. I didn’t even know about this app three days until the exam and it has helped A LOT. Please actually trust me and use it as I’m sure you too will see developments.
Xander S
iOS user
THE QUIZES AND FLASHCARDS ARE SO USEFUL AND I LOVE THE SCHOOLGPT. IT ALSO IS LITREALLY LIKE CHATGPT BUT SMARTER!! HELPED ME WITH MY MASCARA PROBLEMS TOO!! AS WELL AS MY REAL SUBJECTS ! DUHHH 😍😁😲🤑💗✨🎀😮
Elisha
iOS user
This apps acc the goat. I find revision so boring but this app makes it so easy to organize it all and then you can ask the freeeee ai to test yourself so good and you can easily upload your own stuff. highly recommend as someone taking mocks now
Paul T
iOS user