Find the molarity of a monoprotic acid for a titration in which 20.00mL of the aqueous...

Question

Question

Find the molarity of a monoprotic acid for a titration in which 20.00mL of the aqueous acid is titrated with 13.36mL of 0.2052 M NaOH.

Answer 1

Answer #1

reaction : HA + NaOH ---------------------> NaA + H2O

it is 1 : 1 reaction

M1 V1 (for base ) = M2 V2 (for acid)

0.2052 x 13.36 = M2 x 20.00

M2 = 0.1371 M

molarity of monoprotic acid = 0.1371 M

Add a comment

Answer 2

Similar Homework Help Questions

Titration of a Weak Monoprotic Acid with a Strong Base Volume of Base (mL) 1. Using...

Titration of a Weak Monoprotic Acid with a Strong Base Volume of Base (mL) 1. Using the graph, determine the K, of the weak acid. 2. Suppose 100mL of the monoprotic acid referred to in the graph was titrated with 1M NaOH, determine the molarity of the weak acid. The corresponding balanced chemical equation is shown below. HA + NaOH + H2O + A + Nat 3. If the weak acid above was prepared by using 5g of the weak...
Weak Acid Titration When a 14.0 mL sample of a monoprotic weak acid is titrated with...

Weak Acid Titration When a 14.0 mL sample of a monoprotic weak acid is titrated with 0.10 M NaOH, it generates the titration curve shown below. Weak Acid titrated with 0.10 M NaOH pH Volume of 0.10 M NaOH a) What is the molar concentration of the original sample of weak acid? х М b) What is the ka for this weak acid?
A titration of a 75.0 mL aqueous solution of 0.12 M acetic acid, a weak, monoprotic...

A titration of a 75.0 mL aqueous solution of 0.12 M acetic acid, a weak, monoprotic acid with a Ka of 1.76 × 10–5, with 0.30 M NaOH is performed. What is the pH of the solution after 10.0 mL of NaOH has been added (at 25oC)? Group of answer choices 5.24 3.98 8.21 6.17 4.45

5.00 mL of a solution containing a monoprotic acid was placed in a 100-mL volumetric flask,...

5.00 mL of a solution containing a monoprotic acid was placed in a 100-mL volumetric flask, diluted to the mark with deionized water and mixed well. Then, 25.00 mL of this diluted acid solution was titrated with 0.08765 M NaOH. 9.23 mL of NaOH was required to reach the endpoint. a. What does the term monoprotic mean? b. Determine the molar ratio between the acid and NaOH. c. Calculate the moles of NaOH used in this titration. d. Calculate the...
3) A weak monoprotic acid has a pKa 6.15. 50.00 mL of an 0.1250M aqueous solution...

3) A weak monoprotic acid has a pKa 6.15. 50.00 mL of an 0.1250M aqueous solution of this weak acid is titrated with 0.1000M NaOH. a) What is the equivalence point volume and 2 equivalence point volume for this titration? Find the pH b) before the titration begins; c) after 20.00 mL of the NAOH has been added, d) after 62.50 mL of the NaOH has been added; and e) after 85.00 mL of the NAOH has been added. 4)...
QUESTION 3 A solution of acetic acid, HC2H302, a weak monoprotic acid, was standardized by titration...

QUESTION 3 A solution of acetic acid, HC2H302, a weak monoprotic acid, was standardized by titration with 0.1660 M NaOH solution. If 20.59 mL of the NaOH were required to neutralize completely 18.23 ml of the acetic acid solution, what is the molarity o of the acetic acid solution?

could i see the steps for these 3 questions ? thank you ! Acid/Base Titration Problems...

could i see the steps for these 3 questions ? thank you ! Acid/Base Titration Problems 6. 20.0 mL of HNO, is titrated with 0.10 M NaOH. After adding 70.0 mL of NaOH, it turned pink. What is the molarity of nitric acid? 7. Ascorbic acid is titrated to an endpoint by 14.5 mL of 0.467 M NaOH. How many mg of ascorbic acid are in each pill? (MW of ascorbic acid = 176.1 g/mol) *Hint: ascorbic acid is monoprotic...
Consider a titration of 20.00mL cyanic acid solution (Ka=3.5x10^-4) with 0.1082 M solution of sodium hydroxide....

Consider a titration of 20.00mL cyanic acid solution (Ka=3.5x10^-4) with 0.1082 M solution of sodium hydroxide. The volume of 21.70 mL of NaOH(aq) was needed to reach the equivalence point. Calculate: a) the concentration of the cyanic acid solution before the titration b) the pH of the cyanic acid solution before the titration c) the pH of the solution at half-equivalence point
In a titration experiment, 11.7 mL of an aqueous H2SO4 solution was titrated with 0.4 M...

In a titration experiment, 11.7 mL of an aqueous H2SO4 solution was titrated with 0.4 M NaOH solution. The equivalence point in the titration was reached when 10.7 mL of the NaOH solution was added. What is the molarity of the H2SO4 solution? H2SO4 molarity

8. Molarity a) The molarity of an aqueous solution of sodium hydroxide, is determined by titration...

8. Molarity a) The molarity of an aqueous solution of sodium hydroxide, is determined by titration against an M hydrochloric acid, solution. If 35.3 mL of the base are required to neutralize 18.2 mL of hydrochloric acid, what is the molarity of the sodium hydroxide solution? Molarity = __________ M b) An aqueous solution has a hydroxide ion concentration of M. What is the hydronium ion concentration in this solution? Concentration = _____M Is this solution acidic, basic or neutral?...