Concept explainers
Interpretation:
The
pH definition:
The concentration of hydrogen ion is measured using
The
On rearranging, the concentration of hydrogen ion
Answer to Problem 6H.2AST
The
Explanation of Solution
The initial amount of
The amount of
Therefore, the
From the stoichiometric point the amount of
The amount of
Hence, the amount of
The total volume of the solution at the stoichiometric point is calculated as,
The concentration of
Therefore, the concentration of
The chemical equilibrium reaction is given below.
Initial concentration | 0.007 | 0 | 0 |
Change in concentration | -x | +x | +x |
Equilibrium concentration | 0.007-x | x | x |
The equilibrium concentration values are obtained in the above table and is substituted in above equation and is given below.
The above equation, assume that the x present in 0.007-x is very small than 0.007 then it can be negligible and it follows,
Hydrochlorous acid
Therefore, the
Hence, the concentration of
Now, we can calculate the pH of the solution,
Hence, the
Want to see more full solutions like this?
Chapter 6 Solutions
CHEMICAL PRINCIPLES (LL) W/ACCESS
- Calculate the solubility in grams per 100 mL of BaF2 in a 0.10 M BaCl2 solution.arrow_forwardCalculate the pH of 0.225 M RbOH(aq).arrow_forwardThe pH of 0.40 M HF(aq) is 1.93. Calculate how the pH changes when 0.356 g of sodium fluoride is added to 50.0 mL of the solution. Assume that the volume change is small and can be neglectedarrow_forward
- Calculate the pH of a solution prepared by dissolving 2.05 g of sodium acetate, CH3COONa, in 71.0 mL of 0.10 M acetic acid, CH3COOH(aq). Assume the volume change upon dissolving the sodium acetate is negligible. Ka of CH3COOH is 1.75 x 10 ^ -5 "Please provide detailed solution and give the explanation of each point"arrow_forwardCalculate the change in pH that results from adding 0.160 M NaNO3 to 1.00 L of 0.160 HNO3 (aq).arrow_forwardCalculate the pH of a 0.055 M AlCl3 (aq) (aluminum chloride) solution. Ka for Al3+ is 1.2 × 10–5.arrow_forward
- A solution of 1.7×10−6 M HNO3(aq) (10.0 mL) is diluted to 10.0 L with pure deionized water at 25 °C . What is the pH of the resulting solution?arrow_forwardConsider 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_forwardCalculate the ph of a solution prepared by dissolving 1.00g of sodium acetate,CH^3COONa, in 50.0ml of 0.15 M acetate acid, CH^3COOH(aq)arrow_forward
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningPrinciples of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning