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Calculate the pH of the final equilibrium mixture in each of the following solutions: 1. 10 mL...

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Chemistry

Calculate the pH of the final equilibrium mixture in each of thefollowing solutions:

1. 10 mL of 0.005 M HNO3 are mixed with 5 mL of 0.006M NaOH [answer: pH=2.87]

2. One mole of HCl is mixed with one mole of ammonia(NH3; kb=1.76*10-5) to form oneliter aqueous solution. [answer: pH=4.62]

3. 0.5 moles of HCl is mixed with one mole of ammonia(NH3; kb=1.76*10-5) to form oneliter aqueous solution. [answer: pH=9.24]

4. One mole of hydrocyanic acid (HCN;ka=6.2*10-10) is mixed with one mole ofpotassium hydroxide (KOH) to form a one liter aqueous solution.[answer: pH=11.60]

5. One mole of hydrocyanic acid (HCN;ka=6.2*10-10) is mixed with 0.5 mole ofpotassium hydroxide (KOH) to form a one liter aqueous solution.[answer: pH=9.21]

6. 0.35 moles of ammonia (NH3;kb=1.76*10-5), 01. mole ammonium nitrate(N3H4O3), and 0.2 mole nitric acidare mixed to form one liter aqueous solution. [answer: pH=8.93]

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