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Chapter 4: Q86E (page 224)

Sodium bicarbonate (baking soda), NaHCO3, can be purified by dissolving it in hot water (60掳C), filtering to remove insoluble impurities, cooling to 0 掳C to precipitate solid NaHCO3 , and then filtering to remove the solid, leaving soluble impurities in solution. Any NaHCO3 that remains in solution is not recovered. The solubility of NaHCO3 in hot water of 60 掳C is 164 g/L. Its solubility in cold water of 0 掳C is 69 g/L. What is the percent yield of NaHCO3 when it is purified by this method?

Short Answer

Expert verified

The percent yield of sodium bicarbonate when purified by the given will be 58%

Step by step solution

01

Given Data

It is given that the solubility of sodium bicarbonate in hot water is 164 g/L which is the theoretical yield of \({\rm{NaHC}}{{\rm{O}}_3}\)

Now, we know that solubility means the solute is dissolved in the solution, and in cold water the \({\rm{NaHC}}{{\rm{O}}_3}\) is present along with the other impurities, so the amount of \({\rm{NaHC}}{{\rm{O}}_3}\) that is present in the solution or the actual yield of \({\rm{NaHC}}{{\rm{O}}_3}\) will be 164 鈥� 69 = 95 g/L

02

Percent yield of sodium bicarbonate

The net percentage yield of the compound is calculated by:

\({\rm{Percentage yield = }}\frac{{{\rm{Actual yield}}}}{{{\rm{Theoretical yield}}}}{\rm{ }} \times {\rm{ 100}}\)

Therefore, the percentage yield of the \({\rm{NaHC}}{{\rm{O}}_3}\) is

\({\rm{Percentage yield = }}\frac{{95}}{{164}}{\rm{ }} \times {\rm{ 100 = 58 percent}}\)

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Most popular questions from this chapter

Titration of a 20.0-mL sample of acid rain required 1.7 mL of 0.0811MNaOH to reach the end point. If we assume that the acidity of the rain is due to the presence of sulfuric acid, what was the concentration of sulfuric acid in this sample of rain?

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?

What is the percent of chloride ion in a sample if 1.324g of sample produces 1.0881g of AgCl when treated with excess Ag+\(A{g^ + } + C{l^ - } \to AgCl\)

Assign oxidation state to elements whose atoms are underlined in each of the following compounds or ions:

  1. KNO3
  2. AlH3
  3. NH4+
  4. H2PO4-

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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