How many moles of HCl need to be added to 200.0 mL of a 0.200 M solution of NaF to make a buffer with a pH of 3.50? (Ka for HF is 6.8 × 10-4)

For 480.0 mL of a buffer solution that is 0.120 M in HC2H3O2 and 7.50×10−2 M in NaC2H3O2 , calculate the initial pH and the final pH after adding 1.5×10−2 mol of HCl . ( Ka(HC2H3O2)=1.8×10−5 .)

What is the pH of a buffer solution that is 0.214 M in ammonia and 0.390 M in ammonium chloride (NH4CI)? The Kü of ammonia is 1.8 x 10-5. (Two decimal places)

Consider a buffer made from 255 mL 0.10M HC2H:O2 and 125 mL 0.10 NaC2H:O2. Ka for HC2H3O2 is 1.8 x 105. Choose the true statement. A) Adding 25 mg NaOH (s) will reduce the pH. B) Adding 25 mL water will increase the pH. C) Adding 25 mL 0.0050 M HCI will increase the pH. D) Adding 25 mL 0.0050 M HF will reduce the pH. E) Adding 25 mg NaCl (s) will increase the pH.

A buffer is made by adding 19.4 grams of lithium fluoride to 200.0 mL of 2.00M HF. a) What is the pH of this system before any strong acid or base is added? b) What is the pH after the addition of 200.0 mL of 0.500M HCl? c)What is the pH after the addition of 400.0 mL of 0.500M HCl?

A 1.0 liter solution contains 0.745 M hydrogen fluoride (HF) and 0.786  M sodium fluoride (NaF).  What is the pH of this solution? (Ka for HF is 7.2 x 10 –4) How many moles of solid sodium acetate would have to be added to 2.0 L of 0.293  M acetic acid solution to achieve a buffer of pH 4.77? Assume there is no volume change.      Ka for HC2H3O2 is 1.8  × 10 –5 What molar ratio of sodium acetate to acetic acid,  is required to create a buffer solution having a pH of 4.58 at 25°C?     Ka for HC2H3O2 is 1.8  × 10 –5.

Moly Cule is titrating 0.2 M of a strong base (NaOH) into 100 ml of a solution of 0.1M weak acid (HAc). Ka for HAc is1.8x10 -5.  How much NaOH must be added to reach the equivalence point, and what is the pH at the equivalence point?

Let’s build a buffer using hypobromous acid (HBrO, Ka = 2.3×10−9) and hypobromite ion (BrO−). If [HBrO] is 0.100 M, then what concentration of hypobromite ion is needed to achieve pH = 8.50

A buffer solution is 0.462 M in HCN and 0.283 M in KCN. If Ką for HCN is 4.0 × 10-¹0, what is the pH of this buffer solution? pH =

a) Calculate the pH of a solution containing 0.30 M HF and 0.30 M NaF.The Ka for HF is 7.2×10-4. pH =  b)  Carbonate buffers are important in regulating the pH of blood at 7.40. If the carbonic acid concentration in a sample of blood is 0.0014 M, determine the bicarbonate ion concentration required to buffer the pH of blood at pH = 7.40. Ka = 4.3×10-7 Сoncentration =  M c) You have 75.0 mL of 0.10 M HA. After adding 30.0 mL of 0.10 M NaOH , the pH is 5.50. What is the Ka  value of HA ?  =  d) Consider the titration of 80.0 mL of 0.100 M Ba(OH)2 by 0.400 M HCl. Calculate the pH of the resulting solution after the following volumes of HCl have been added. 40.0 mL pH =  50.0 mL pH =