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Chapter 4: Q94E (page 225)

Potassium acid phthalate, KHC6H4O4or KHP, is used in many laboratories, including general chemistry laboratories, to standardize solutions of base. KHP is one of only a few stable solid acids that can be dried by warming and weighed. A 0.3420-g sample of KHC6H4O4 reacts with 35.73 mL of a NaOH solution in a titration. What is the molar concentration of the NaOH?

\({\rm{KH}}{{\rm{C}}_6}{{\rm{H}}_4}{{\rm{O}}_{4({\rm{aq}})}}{\rm{ + NaO}}{{\rm{H}}_{({\rm{aq}})}}{\rm{ }} \to {\rm{ KNa}}{{\rm{C}}_6}{{\rm{H}}_4}{{\rm{O}}_{4({\rm{aq}})}}{\rm{ + }}{{\rm{H}}_2}{{\rm{O}}_{({\rm{aq}})}}\)

Short Answer

Expert verified

The molar concentration of sodium hydroxide is \({\rm{5}}{\rm{.3 }} \times {\rm{ 1}}{{\rm{0}}^{ - 3}}\;{\rm{M}}\)

Step by step solution

01

Moles of sodium hydroxide

According to the question, it is given that

The mass of KHC6H4O4 is 0.3420 g

The molecular mass of KHC6H4O4 is \(39\,{\rm{ + }}{\rm{5 }} \times {\rm{ 1 + }}{\rm{12 }} \times {\rm{ 6 + }}{\rm{16 }} \times {\rm{ }}4\;{\rm{ = 180 g/mol}}\)

Thus, the number of moles of KHC6H4O4 will be given by:

\(\begin{array}{l}{\rm{Moles = }}\frac{{{\rm{Mass}}}}{{{\rm{Molecular mass}}}}\\{\rm{Moles = }}\frac{{0.3420}}{{{\rm{180}}}}{\rm{ = 0}}{\rm{.0019 moles}}\end{array}\)

Now, from the reaction we can determine that when 1 mole of KHC6H4O4 reacts with sodium hydroxide it requires 1 mole of NaOH, thus the number of moles of sodium hydroxide will be:

\({\rm{1 }} \times {\rm{ 0}}{\rm{.0019 = 0}}{\rm{.0019 moles}}\)

02

Molar concentration of sodium hydroxide

The molar concentration of a compound, also known as molarity, is a method of determining the concentration of a substance in a solvent. As the number of moles of sodium hydroxide is 0.0019 moles and the volume is 35.73 ml. Thus, the molar concentration of sodium hydroxide is given by:

\(\begin{array}{l}{\rm{Concentration = }}\frac{{{\rm{Moles}}}}{{{\rm{Volume}}}}\\{\rm{Concentration = }}\frac{{0.0019}}{{35.73}}{\rm{ = 5}}{\rm{.3 }} \times {\rm{ 1}}{{\rm{0}}^{ - 3}}\;{\rm{M}}\end{array}\)

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Most popular questions from this chapter

What is the concentration of NaCl in a solution if titration of 15.00 mL of the solution with 0.2503MAgNO3 requires 20.22 mL of the AgNO3 solution to reach the end point?

AgNO3(aq) + NaCl(aq)鉄禔驳颁濒(s) + NaNO3(aq)

Use the following equations to answer the next four questions:

i.\({H_2}O\left( s \right) \to {H_2}O\left( l \right)\)

ii.\(N{a^ + }\left( {aq} \right) + C{l^ - }\left( {aq} \right) + A{g^ + }\left( {aq} \right) + NO_3^ - \left( {aq} \right) \to AgCl\left( s \right) + N{a^ + }\left( {aq} \right) + NO_3^ - \left( {aq} \right)\)

iii.\(C{H_3}OH\left( g \right) + {O_2}\left( g \right) \to C{O_2}\left( g \right) + {H_2}O\left( g \right)\)

iv. \(2{H_2}O\left( l \right) \to 2{H_2}\left( g \right) + {O_2}\left( g \right)\)

v. \({H^ + }\left( {aq} \right) + O{H^ - }\left( {aq} \right) \to {H_2}O\left( l \right)\)

(a) Which equation describes a physical change?

(b)Which equation identifies the reactants and products of a combustion reaction?

(c)Which equation is not balanced?

(d)Which is a net ionic equation?

Outline the steps needed to determine the limiting reactant when 0.50 mol of Cr and 0.75 mol of H3PO4 react according to the following chemical equation.\(2Cr + 2{H_3}P{O_4} \to 2CrP{O_4} + 3{H_2}\). Determine the limiting reactant.

A 0.025-g sample of a compound composed of boron and hydrogen, with a molecular mass of ~28 amu, burns spontaneously when exposed to air, producing 0.063 g of B2O3. What are the empirical and molecular formulas of the compound?

Write a balanced equation describing each of the following chemical reactions.

(a) Solid potassium chlorate, KClO3 decomposes to form solid potassium chloride and diatomic oxygen gas

(b) Solid aluminium metal reacts with solid diatomic iodine to form solid Al2I6

(c) When solid sodium chloride is added to aqueous sulfuric acid, hydrogen chloride gas and aqueous sodium sulfate are produced.

(d) Aqueous solutions of phosphoric acid and potassium hydroxide react to produce aqueous potassium dihydrogen phosphate and liquid water.
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