A sample of soda ash (impureNa2CO3) is titrated with 0.5000 NH2SO4. If the sample weighs 1.1000g requires 35.00 mL of the acid forcomplete neutralization, what is the%Na2CO3 in the ash assuming noother active component is present? (;Na 22.99, C 12.01, O 16.00, H 1.008, S32.07)

Given, Mass of sample = 1.10 g Molar mass of Na2CO3 = 106 g/mol Normality of H2SO4 = 0.500 N…

2CO3) is titrated with 0.5000 N SO4. If the sample weighs 1.100 equires 35.00 mL of the acid fo mplete neutralization, what is t Na2CO3 in the ash assuming nơ her active component is presen 22.99, C 12.01, O 16.00, H 1.008 07)

2CO3) is titrated with 0.5000 N SO4. If the sample weighs 1.100 equires 35.00 mL of the acid fo mplete neutralization, what is t Na2CO3 in the ash assuming nơ her active component is presen 22.99, C 12.01, O 16.00, H 1.008 07)

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.26QAP

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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

A sample of soda ash (impure
Na2CO3) is titrated with 0.5000 N
H2SO4. If the sample weighs 1.1000
g requires 35.00 mL of the acid for
complete neutralization, what is the
%Na2CO3 in the ash assuming no
other active component is present? (;
Na 22.99, C 12.01, O 16.00, H 1.008, S
32.07)

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