Calculate the pH of the solution that results when 15.0 mL of 0.1790 M formic acid (Ka(HCOOH) = 1.80 × 10-4a. diluted to 45.0 mL with distilled water.pH =b. mixed with 30.0 mL of 0.0895 M NaOH solution.pHc. mixed with 30.0 mL of 0.150 M NaOH solution.pH =d. mixed with 30.0 mL of 0.150 M sodium formate solution.pH =

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Answered: Calculate the pH of the solution that…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.29QAP

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A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
1. the temperature for each solution is carried out at approximately 297 K where Kw = 1.00 x 10 ^-14 (a) 0.20 g of hydrogen chloride (HCl) is dissolved in water to make 4.5 L of solution. What is the pH of the resulting hydrochloric acid solution? (b) 0.70 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 3.0 L of solution. What is the pH of this solution ?
Determine how much of each acid and conjugate base are needed to add to a final volume of 500ml of Distilled water to prepare a ph of 7.5? Molarity=0.200 pka=7.20 dibasic MW=120 Monobasic MW=200..
1. Write a chemical equation for the dissociation of the hypochlorite ion, ClO-1, in water to make a basic solution. 2. The Ka for benzoic acid (HC7H5O2), is 6.5 x 10-5. Calcuklate pH of a 0.10 M benzoic acid solution. 3. Calculate the pH of a 0.24 M solution of weak base A-1 that has a Kb of 2.5 x 10-6.
Propionic acid, HC3H5O2, has Ka= 1.34 x 10–5. (a) What is the molar concentration of H3O+ in 0.15 M HC3H5O2 and the pH of the solution? (b) What is the Kb value for the propionate ion, C3H5O2–? (c) Calculate the pH of 0.15 M solution of sodium propionate, NaC3H5O2. (d) Calculate the pH of solution that contains 0.12 M HC3H5O2 and 0.25 M NaC3H5O2.
Calculate ph of a 0.94 M solution of a weak base with KB= 1.97 x 10^-9
Calculate the pH of a solution that has an ammonium chloride concentration of 0.058 M and an ammonia concentration of 0.052 M. Kb= 1.8 x 10^-5
The temperature for each solution is carried out at approximately 297 K where Kw=1.00×10−14. a) 0.60 g of hydrogen chloride (HCl) is dissolved in water to make 5.5 L of solution. What is the pH of the resulting hydrochloric acid solution? b) 0.45 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 4.5 L of solution. What is the pH of this solution?
Determine pH of a solution containing 0.320 M C3H7NH2 and 0.140 M NaBr if Kb of C3H7NH2 is 2.17 x 10-5
What is the pH of a solution that is 0.32 M H(C6H5COO) and 0.12 M Na(C6H5COO)? The Ka of H(C6H5COO) is 6.3 x 10-5
What is the theoretical pH of 0.10 M CH3COOH? The Ka of CH3COOH is 1.8 x 10-5
13.3.00 g of pure acetic acid (CH3COOH) is diluted to 25.0 L, What is the PH of the solution? Ka = 1.8 x 10-5

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Calculate the pH of the solution that results when 15.0 mL of 0.1790 M formic acid ( Ka(HCOOH) = 1.80 × 10¬4) is %3D a. diluted to 45.0 mL with distilled water. pH = b. mixed with 30.0 mL of 0.0895 M NaOH solution. pH = c. mixed with 30.0 mL of 0.150 M NaOH solution. pH =