Part A Calculate the pH of a buffer solution that contains 0.900 M CH3NH2 and 1.10 M CH3NH3CI. (Kb = 4.4×10-4). pH of buffer = Part B 85.0 mL of 0.950 M NaOH is added to 250.0 mL of the buffer solution described in Part A. What is the pH of the solution after the NaOH(aq) is added? pH after NaOH added = Part C 80.0 mL of 0.800 M HNO3 is added to 250.0 mL of the buffer solution described in Part A. What is the pH of the solution after the HNO3 is added? pH after HNO3 added =

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A: Answer is explained below.

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A: We have to calculate the concentration of the conjugate base in final solution.

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Q: Calculate the pH of a buffer solution that contains 0.950 M CH3NH2 and 1.00 M CH3NH3Cl. (Kb =…

A: Since you have posted a question with multiple independent parts, we will solve first part for you.…

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Q: OHI(aq) + NH4OH(aq) = H₂O(l) + NH4l(aq) O H3O+ (aq) + NH4OH(aq) = H₂O(l) + NH4+ (aq) O HI(aq) +…

A: •STRONG ACID:- Acid which dissociate completely in solution are called strong acid. :-EXAMPLE:- HI,…

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Q: NH,*(aq)²NH,(aq) + H*(aq)

A:

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Q: what is the molarity of the phosphoric acid?

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.