How many grams of Ca(NO2)2 must be added to 4.0 L solution of 0.1 M HNO2 to get a pH of 3.64?
Solution:
The balanced chemical rection is,
2 HNO2 + Ca(OH)2 = Ca(NO2)2 + 2 H2O
Molar mass of Ca(OH)2 = 74.093 g/mol
Molar mass of Ca(NO2)2 = 132.089 g/mol
Molar mass of HNO2 = 47.013 g/mol
molar mass of water = 18 g/mol
[HNO2] = 0.1 M pH = 3.64 --> [H+] = 10-3.64 = 0.000229 M
Molarity = Moles / Volume in Litre
0.000229 = (Ca(NO2)2 in grams / 132.089) / 4.0 L
Ca(NO2)2 in grams = 0.12 grams
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