Consider a water sample in a closed system with Cr,c03-8x10-4 M and pH=8. a) What is the alkalinity of this water sample? b) How much acid is required to reduce the pH of the sample to 6 assuming no exchange of CO₂(g) with the atmosphere (i.e., the system stays closed)? c) What would be the pH of the sample if it came to equilibrium with the atmosphere (Pc02-10-3.5 atm)? Hint: recall that CO₂(g) → CO₂ (aq) has KH-10-¹.5 and [u,co;]= [co,(aq)].
Consider a water sample in a closed system with Cr,c03-8x10-4 M and pH=8. a) What is the alkalinity of this water sample? b) How much acid is required to reduce the pH of the sample to 6 assuming no exchange of CO₂(g) with the atmosphere (i.e., the system stays closed)? c) What would be the pH of the sample if it came to equilibrium with the atmosphere (Pc02-10-3.5 atm)? Hint: recall that CO₂(g) → CO₂ (aq) has KH-10-¹.5 and [u,co;]= [co,(aq)].
Chemistry
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Only part C please!!
![**Water Sample Analysis in a Closed System**
Consider a water sample in a closed system with a total carbonate concentration \( C_{T, CO_3} = 8 \times 10^{-4} \, \text{M} \) and a pH of 8.
a) **What is the alkalinity of this water sample?**
Alkalinity is a measure of the ability of the water to neutralize acids. It is generally composed of bicarbonates \( \text{HCO}_3^- \), carbonates \( \text{CO}_3^{2-} \), and occasionally hydroxides \( \text{OH}^- \).
b) **How much acid is required to reduce the pH of the sample to 6 assuming no exchange of \( \text{CO}_2(g) \) with the atmosphere (i.e., the system stays closed)?**
Determine the amount of protons (\( \text{H}^+ \)) needed to shift the pH from 8 to 6. Consider the buffer system involves carbonates and bicarbonates.
c) **What would be the pH of the sample if it came to equilibrium with the atmosphere (\( P_{CO_2} = 10^{-3.5} \, \text{atm} \))? Hint: recall that \( \text{CO}_2(g) \leftrightarrow \text{CO}_2(aq) \) has \( K_H = 10^{-1.5} \) and \( [H_2CO_3^*] \approx [CO_2(aq)] \).**
Calculate the equilibrium concentration of dissolved carbon dioxide and evaluate how it influences the pH. Consider the equilibrium constant and partial pressures involved to find the new pH upon reaching equilibrium with the atmosphere.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc52b3a7d-5814-4bdd-8c26-96eede61577b%2F919eb221-f459-408a-b486-af703207d3ee%2F9uxqo97_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Water Sample Analysis in a Closed System**
Consider a water sample in a closed system with a total carbonate concentration \( C_{T, CO_3} = 8 \times 10^{-4} \, \text{M} \) and a pH of 8.
a) **What is the alkalinity of this water sample?**
Alkalinity is a measure of the ability of the water to neutralize acids. It is generally composed of bicarbonates \( \text{HCO}_3^- \), carbonates \( \text{CO}_3^{2-} \), and occasionally hydroxides \( \text{OH}^- \).
b) **How much acid is required to reduce the pH of the sample to 6 assuming no exchange of \( \text{CO}_2(g) \) with the atmosphere (i.e., the system stays closed)?**
Determine the amount of protons (\( \text{H}^+ \)) needed to shift the pH from 8 to 6. Consider the buffer system involves carbonates and bicarbonates.
c) **What would be the pH of the sample if it came to equilibrium with the atmosphere (\( P_{CO_2} = 10^{-3.5} \, \text{atm} \))? Hint: recall that \( \text{CO}_2(g) \leftrightarrow \text{CO}_2(aq) \) has \( K_H = 10^{-1.5} \) and \( [H_2CO_3^*] \approx [CO_2(aq)] \).**
Calculate the equilibrium concentration of dissolved carbon dioxide and evaluate how it influences the pH. Consider the equilibrium constant and partial pressures involved to find the new pH upon reaching equilibrium with the atmosphere.
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