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# Titration of Seawater

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1. Write the complete ionic and net ionic equations for the reaction between AgNO3 and K2CrO4.
Molecular equation: 2AgNO3 (aq) + K2CrO4 (aq) Ag2CrO4 (s) + 2KNO3 (aq)

2. Write the complete ionic and net ionic equations for the reaction between AgNO3 and NaCl.
Molecular equation. AgNO (aq)+NaCl(aq)---à AgCl(s)+NaNO (aq)

3. The 125 mL flask can be wet when the 25 mL of seawater is added using the volumetric pipet. Why doesn't the water in the flask cause problems in the calculations?

4 A technician wants to prepare a standard solution of silver nitrate. The concentration of the solution needed is 0.0750 mol/L with a volume of 1000 mL. Explain and calculate how the technician should prepare this solution

##### Solution Summary

This solution explains several key questions dealing with the titration of seawater:

1) How to write ionic and net ionic equations.
2) How excess water in a titration will affect the results.
3) How to prepare a standard solution.

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titration of seawater
1. Write the complete ionic and net ionic equations for the reaction between AgNO3 and K2CrO4.
Molecular equation: 2AgNO3 (aq) + K2CrO4 (aq) Ag2CrO4 (s) + 2KNO3 (aq)

In an ionic equation, any aqueous (aq) compound will break apart into its relative ions:
2 Ag+ (aq) + 2 NO3- (aq) + 2 K+ (aq) + CrO4- (aq)  Ag2CrO4 (s) + 2 K+ (aq) + 2 NO3- (aq)
In a net ionic equation, you will cross off any ions that appear on both sides of the reaction arrow:
2 Ag+ (aq) + 2 NO3- (aq) + 2 K+ (aq) + CrO4- (aq)  Ag2CrO4 (s) + 2 K+ (aq) + 2 NO3- (aq)
2 Ag+ (aq) + CrO4- (aq) ...

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