Question

The pH of a solution containing 49.0 mL of 0.10 M KOH and 50.0 mL of...

The pH of a solution containing 49.0 mL of 0.10 M KOH and 50.0 mL of 0.10 M of HBr is:

a. 5.0 b. 3.0 d. 7.0 e. 4.0

Homework Answers

Answer #1

answer : b ) 3.0

solution:

millimoles of KOH = 49.0 x 0.10 = 4.90

millimoles of HBr = 50 x 0.1 = 5

millimoles of acid > millimoles of base

after reaction millimoles of acid remains = 5- 4.9 = 0.1

molarity of [H+] = 0.1 / total volume

                          = 0.1 / (49 +50)

                        = 1.0 x 10^-3 M

pH = -log [H+]

pH = -log (1.0 x 10^-3)

pH = 3.0

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH...
A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 13.0 mL of KOH.
A solution containing an unknown concentration of HBr was titrated with 0.100 M KOH. 25.00 mL...
A solution containing an unknown concentration of HBr was titrated with 0.100 M KOH. 25.00 mL of the HBr solution was pipetted into a beaker. The HBr solution was then titrated with the 0.100 M KOH and 18.60 mL of KOH was added to reach the end point. Calculate the concentration of the HBr in the original solution
Determine the pH of the following solution: A 1.0 L of an aqueous solution containing 3.0...
Determine the pH of the following solution: A 1.0 L of an aqueous solution containing 3.0 grams of HBr and 7.0 mL of 1.0 M NaOH.
What is the pH when 30.0 mL of 0.10 M HCOOH solution is titrated with 10.0...
What is the pH when 30.0 mL of 0.10 M HCOOH solution is titrated with 10.0 mL of 0.20 M NaOH? (Ka=1.8 x 10−4) Which of the following titration curves would give the sharpest equivalence point? A 0.1 M HOBr with 0.1 M KOH B 0.1 M HOBr with 0.1 M NH3 C 0.1 M HBr with 0.1 M KOH D 0.1 M HBr with 0.1 M NH3
Q: A 50 mL solution containing 0.10 M 1-Naphtoic acid (pKa = 3.70) and 0.15 M...
Q: A 50 mL solution containing 0.10 M 1-Naphtoic acid (pKa = 3.70) and 0.15 M arsenic acid (pKa1 = 2.24; pKa2 = 6.96) is titrated with 0.20 M KOH. a. How many end points will be observed? b. What is the pH of the solution before adding any KOH? c. Calculate the volume of KOH required to reach the first equivalence point. d. Calculate the pH after the addition of 100 mL of KOH (assume that the OH-contribution from...
What is the pH of a solution of 50.0 mL of 0.112 M NaOH that has...
What is the pH of a solution of 50.0 mL of 0.112 M NaOH that has been titrated with 36.0 mL of 0.350 M HBr?
Calculate the pH for each of the following cases in the titration of 50.0 mL of...
Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.210 M HClO(aq) with 0.210 M KOH(aq). The ionization constant for HClO 4.0*10^-6 a. before any KOH b. After addition of 25 ml of KOH c. After addition of 30 ml of KOH d. After addition of 50 ml of KOH e. After addition of 60 ml of KOH
QUESTION 7 What is the pH of a solution made by mixing 30.00 mL of 0.10...
QUESTION 7 What is the pH of a solution made by mixing 30.00 mL of 0.10 M HCl with 40.00 mL of 0.10 M KOH? Assume that the volumes of the solutions are additive. 0.85 1.85 12.15 13.15 1 points (Extra Credit)    QUESTION 8 Which of the following titrations result in a basic solution at the equivalence point? HI titrated with NaCH3CO2 HOCl titrated with NaOH HBr titrated with KOH HNO3 titrated with NH3
What is the pH of a solution containing 0.10 M sodium acetate to which is added...
What is the pH of a solution containing 0.10 M sodium acetate to which is added 0.10 M acetic acid? What is the pH of a solution prepared by mixing 40 ml of 0.10 M acetic acid with 60 ml of 1 M sodium acetate?
If 10.0 mL of 0.20 M NaOH is added to 50.0 mL of 0.10 M HCl,...
If 10.0 mL of 0.20 M NaOH is added to 50.0 mL of 0.10 M HCl, what will be the pH of the resulting solution?