A 50.0 mL solution of Ca(OH)$_2$ with an unknown concentration was titrated with 0.340 M HNO$_3$. To reach the endpoint, a total of 28.7 mL of HNO$_3$ was required. Given that 0.00976 mol of HNO$_3$ 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 HNO$_3$. To reach the endpoint, a total of 28.7 mL of HNO$_3$ was required.

Given that 0.00976 mol of HNO$_3$ 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 28.7 mL of HNO3 was required.

Given that 0.00976 mol of HNO3 are used in the titration, What quantity in moles of Ca(OH)2 had to be present in the initial reaction?

Added by Margaret R.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Adi S

07/21/2023

Step 1

The balanced chemical equation is: Ca(OH)$_2$(aq) + 2HNO$_3$(aq) $\rightarrow$ Ca(NO$_3$)$_2$(aq) + 2H$_2$O(l) Show more…

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A 50.0 mL solution of Ca(OH)$_2$ with an unknown concentration was titrated with 0.340 M HNO$_3$. To reach the endpoint, a total of 28.7 mL of HNO$_3$ was required. Given that 0.00976 mol of HNO$_3$ are used in the titration, What quantity in moles of Ca(OH)$_2$ had to be present in the initial reaction? mol