10. A solution is prepared by mixing 500 mL of 1 M HCI with 500 mL of 0.01 M HNO3. What is the pH of the resulting solution? (A) 0.0 (B) between 0.0 and 1.0 (C) 1.0 (D) greater than 1.0 n research proiect a scientist adds 0.1 mole of HCN, In rch

10. A solution is prepared by mixing 500 mL of 1 M HCI with 500 mL of 0.01 M HNO3. What is the pH of the resulting solution? (A) 0.0 (B) between 0.0 and 1.0 (C) 1.0 (D) greater than 1.0 n research proiect a scientist adds 0.1 mole of HCN, In rch

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 40P

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

10. A solution is prepared by mixing 500 mL of 1 M HCI with
500 mL of 0.01 M HNO3. What is the pH of the resulting
solution?
(A) 0.0
(B) between 0.0 and 1.0
(C) 1.0
(D) greater than 1.0
n research proiect
a scientist adds 0.1 mole of HCN,
In
rch

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A student prepares 455 mL of a KOH solution, but neglects to write down the mass of KOH added. His TA suggests that he take the pH of the solution. The pH is 13.33. How many grams of KOH were added?
Consider citric acid, H3C6H5O7, added to many soft drinks. The equilibrium constants for its step-wise ionization areKa1=7.5104 ,Ka2=1.7105, andKa3=4.0107. Write the overall net ionic equation and calculate K for the complete ionization of citric acid.
Benzoic acid (K a=6.6105)is present in many berries. Calculate the pH and % ionization of a 726-mL solution that contains 0.288 mol of benzoic acid.
A solution is made by dissolving 15.0 g sodium hydroxide in approximately 450 mL water. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to bring the volume to 500.0 mL of solution. (a) Calculate the pH and pOH in the final solution. (b) Why would we wait for it to return to room temperature? (c) If the mass of the water used to initially dissolve the sodium hydroxide were exactly 450 g and the temperature of the water increased by 8.865 C, how much heat was given off by the dissolution of 15.0 g of solute? Assume the specific heat of the solution is 4.184 J/g. K. What is the molar heat change for the dissolution of sodium hydroxide (known as the enthalpy of solution, Hsol)?
. Using Fig. 16.3, list the approximate pH value of live “everyday” solutions. How do the familiar properties (such as the sour taste for acids) of these solutions correspond to their indicated pH?
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Calculate the pH change that results when 12 mL of 5.3 M NaOH is added to 768 mL of each the following solutions. (See the Acid-Base Table attached.) (a) pure water (b) 0.10 M NH4Cl (c) 0.10 M NH3(d) a solution that is 0.10 M in each NH4+ and NH3

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