A 50.0 mL solution of Ca(OH)2 with anunknown concentration was titrated with0.340 M HNO3. To reach the endpoint, a totalof 28.4 mL of HNO3 was required.Given that 0.00966 mol of HNO3 are used inthe titration, What quantity in moles ofCa(OH)2 had to be present in the initialreaction?mol13.4C78.+/-х 10LO

Neutralization :- The reaction of an acid with a base to form salt and water is known as…

A 50.0 mL solution of Ca(OH)2 with an unknown concentration was titrated with 0.340 M HNO3. To reach the endpoint, a total of 28.4 mL of HNO, was required. Given that 0.00966 mol of HNO, are used in the titration, What quantity in moles of Ca(OH)2 had to be present in the initial reaction?

A 50.0 mL solution of Ca(OH)2 with an unknown concentration was titrated with 0.340 M HNO3. To reach the endpoint, a total of 28.4 mL of HNO, was required. Given that 0.00966 mol of HNO, are used in the titration, What quantity in moles of Ca(OH)2 had to be present in the initial reaction?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 93QRT: When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence...

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Question

A 50.0 mL solution of Ca(OH)2 with an
unknown concentration was titrated with
0.340 M HNO3. To reach the endpoint, a total
of 28.4 mL of HNO3 was required.
Given that 0.00966 mol of HNO3 are used in
the titration, What quantity in moles of
Ca(OH)2 had to be present in the initial
reaction?
mol
1
3.
4
C
7
8.
+/-
х 10
LO

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