if 10.0 ml of 0.350 m aqueous nano3 is mixed with 50.0 ml of 0.170 m aqueous kno3, what is the molarity of nitrate ion?
a) 0.185 m
b) 0.200 m
c) 0.260 m
d) 0.520 m

0.200 mol/L  

Explanation:

1. Moles of nitrate in first solution

Moles = volume × concentration  

n = 0.0100 L × 0.350 mol/L =0.003 500 mol

2. Moles of nitrate in second solution

n = 0.0500 L × 0.170 mol/L = 0.008 500 mol

3. Total moles of nitrate

n = 0.003 500 + 0.008 500 = 0.012 000 mol

4. Total volume of solution

V = 10.0 + 50.0 = 60.0 mL = 0.0600 L

5. New concentration of nitrate

c = moles/litres

c = 0.012 000 mol/0.0600 L = 0.200 mol/L

The molar concentration of nitrate ion is 0.200 mol/L.

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the answer is 0.8m.

by: nicholas