22. A 100.0-ml buffer solution is 0.175 M in HCIO and 0.150 M in Nacio. a. What is the initial pH of this solution?...
A 100.0 mL buffer solution is 0.175 M in HCIO and 0.150 M in NaCIO. What is the initial pH of this solution? Express your answer using two decimal places. ACO Submit Request Answer Part B What is the pH after addition of 1500 mg of HBr? Express your answer using two decimal places. Yol AXC og
1.) A buffer solution is 0.175 M in HClO and 0.150 M in NaClO. What happens after addition of HBr? A)The amount of ClO- will increase B)The amount of HClO will increase C)The amounts of these components will stay the same D)The amount of HClO will decrease 2.) A 1L buffer solution is 0.175 M in HClO and 0.150 M in NaClO. What is the pH after addition of 0.10 mol HBr? pKa = 7.53 A)6.79 B)7.53 C)8.27 D)9.23
1000 ml buffer is 0.175 M of HClO and 0.150M in HClO and the pH is 7.47 1. what is the pH when 10.00ml of 2.0M NaOH is added? 2. if you add 150mg of HBr what will be the new pH (assume no volume change). Molar mass of HBr is 80.91g/mol sorry HClO it is 0.175 M and for NaClO it is 0.150
4. An aqueous buffer solution if made from 150.0 mL of a 1.50 M HCN solution and 200.0 mL of a 1.00 M NaCN solution. The Ka for HCN is 4.90 x 10-10. a. Calculate the initial pH of this buffer solution. b. Calculate the pH after adding 100.0 mL of 0.800 M HBr to the HCN/NaCN buffer. c. Calculate the pH after adding 100.0 mL of 0.800 M KOH to the HCN/NaCN buffer.
Calculate the pH of a solution formed by mixing 100.0 mL of 0.20 M HCIO with 200.0 mL of 0.30 M NACIO The Ka for HCIO is 2.9 x 10-8 ANSWER: ODA 10/ 7.54 7.06 5.99 6.46 8.01
Calculate the pH for each case in the titration of 50.0 mL of 0.150 M HCIO(aq) with 0.150 M KOH(aq). Use the ionization constant for HCIO. What is the pH before addition of any KOH? pH = What is the pH after addition of 25.0 mL KOH? pH = What is the pH after addition of 30.0 mL KOH? pH = What is the pH after addition of 50.0 mL KOH? pH = What is the pH after addition of...
4. What is the pH of a 100.0 mL buffer solution containing 0.15 M NaHCO3 and 0.15 M Na2CO3? 5. What is the pH after adding 15.0 mL of 0.10 M NaOH to the solution in question 4?
1. You are titrating a 100.0 mL solution of 0.050 M HBrwith a 0.150 M solution of KOH. What will be the pH after the addition of 25.0 mL KOH? 2. You titrate 250 mL of 0.250 M acetic acid (Ka= 1.8 x 10-5) with 50.0 mL of 0.350 M NaOH. What is the pH of this solution? 3. For the titration in question 2, what would be the Kaof an ideal indicator.
Calculate the following: a. The pH of a 500.0 mL buffer solution containing 0.75 M HCN (Ka = 6.2 x 10^-10) and 0.55 M NaCN b. The pH of the above buffer after the addition of 100.0 mL of 1.0 M NaOH. c. The pH of the buffer if 100.0 mL of 1.0 M HCl was added to the solution in part a.
What is the pH at the equivalence point when 85.0 mL of a 0.175 M solution of acetic acid ( CH3COOH) is titrated with 0.100 M NaOH to its end point?