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    pH and pOH problems

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    a) If 0.1 g of Silver Nitrite (AgNO2; Ksp = 6.0 x 10 ^ -4) is added to 100 mL of water, what would the pH and pOH be? Note: The Ka for HNO2 is 7.2 x 10 ^ -4

    b). If 0.1 g of Silver Nitrite is added to 0.1M solution of NaOH, what would the pH be? How much Silver Nitrite would dissolve?

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    https://brainmass.com/chemistry/acids-and-bases/ph-poh-problems-534853

    Solution Preview

    a) AgNO2 ---> Ag+ + NO2 -

    [AgNO2] = (0.1g/154 g) x (1mol / 0.100L) = 6.5 x 10^-3 M = 0.0065M

    Ksp = [Ag+][NO2-] = (s)^2 where 's' is the solubility of AgNO2

    Hence s = 0.0245 M. As solubility is greater than initial concentration of AgNO2, all 0.0065M will dissolve to form ...

    Solution Summary

    Two problems based on the solubility of AgNO2 are solved.

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