Concept explainers
(a)
Interpretation:
The
Concept Introduction:
Henderson – Hasselbalch equation:
The
(a)
Explanation of Solution
Given that, the
By using Henderson – Hasselbalch equation, the initial
The addition of a base will react with the weak acid and thus decreases the concentration of weak acid and increases the concentration of conjugate base.
The reaction of added base with some of
The initial number of moles of acid can be calculated as shown below.
The number of moles of added base can be calculated as shown below.
The molar ratio of acid and added base in the above equation is
Now, the remaining amount of acid can be estimated.
The new concentration of conjugate base can be calculated as shown below.
Now, the
Therefore, the
(b)
Interpretation:
The
Concept Introduction:
Refer to part (a).
(b)
Explanation of Solution
Given that, the
By using Henderson – Hasselbalch equation, the initial
The addition of a strong acid will react with the conjugate base and thus decreases the concentration of conjugate base and increases the concentration of weak acid.
The reaction of added acid with some of
The initial number of moles of acid can be calculated as shown below.
The number of moles of added acid can be calculated as shown below.
The new concentration of weak acid can be calculated as shown below.
The molar ratio of conjugate base and added acid is
Now, the remaining amount of conjugate base can be estimated.
Now, the
Therefore, the
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Chapter 6 Solutions
ACHIEVE/CHEMICAL PRINCIPLES ACCESS 1TERM
- When using a 0.100 M HCl (aq) standard solution and measuring 50 ml of 0.100 M NH3 (aq), Find the pH under each of the following conditions. (a) (a) the initial state before adding the HCl(aq) standard solution; (b) (b) 40.0 ml of HCl(aq) standard solution is added. (c) (c) 50.0 ml of HCl(aq) standard solution is added. (d) (d) 50.2 ml of HCl(aq) standard solution is added.arrow_forwardCalculate the pH of a buffer containing 0.1 M HC2H3O2 (aq) mixed with 0.1 M NaC2H3O2 (aq)?arrow_forward1) Calculate the pH of a solution prepared by dissolving 2.35 g of sodium acetate, CH,COONA, in 81.5 ml of 0.10 Macetic acid, CH,COOH(aq). Assume the volume change upon dissolving the sodium acetate is negligible. K, of CH,COOH is 1.75 x 10. pH=arrow_forward
- Consider the titration of 25.0 mL of 0.112 M acetic acid (CH, COOH, pK, = 4.75) with 0.131 M NaOH. CH;COOH(aq)+NaOH(aq) · CH, COO (aq) + H,O(1) + Na*(aq) Determine the initial pH of the 0.112 M acetic acid solution before NaOH is added. pH : Determine the pH of the solution after 10.0 mL of 0.131 M NaOH is added. pH =arrow_forward650.0 mL of HBr gas at 21.0 °C and 1025 mm Hg is absorbed completely into a solution that was created by mixing 7.147 g of Na2CO3 and 250.0 g of water. (a) What is the pH of the solution? (b) What is the freezing point of the solution?arrow_forwardCalculate the change in pH when 7.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M inNH3(aq) and 0.100 M in NH4Cl(aq). ΔpH= Calculate the change in pH when 7.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution. ΔpH=arrow_forward
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- The solubility of iron(II) hydroxide, Fe(OH)2, is 1.43×10–3 gram per liter at 25 °C. (a) Write a balanced equation for the solubility equilibrium. (b) Write the expression for the solubility product constant, Ksp, and calculate its value. (c) Calculate the pH of a saturated solution of Fe(OH)2 at 25 °C.arrow_forwardDetermine the pH at the equivalence (stoichiometric) point in the titration of 48.38 mL of 0.171 M HCN (aq) with 0.135 M NaOH(aq). The Ka of HCN is 4.9 * 10^-10.arrow_forwardQ.3: Determine the pH of the dissociation of 0.1 M HCN (aq). For which the dissociation constant is equal to 4.9 x 10-5 and the weight and volume of the conjugated base is 5 g and 2 L respectively. (Write the chemical reaction).arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning