A student prepared 100.0 mL of a buffer in the lab that contains 0.300 M of a weak acid, HA, and 0.200 M of its conjugate base, NaA. The student then added 1.0x10- moles of NaOH to the buffer. a) Write down your student name and number b) Write down how the student calculated the final moles of A- and HA after adding the NaOH: moles A Fing =2.0x10 mole - 1.0x10-3mole moles HA Eno= 3.0x10 2mole +1.0x10 3mole c) There is an error in their formula. Identify the error d) Calculate the correct final moles of A and HA

Calculate the pH of a buffer solution containing 0.584 mol HA weak acid and 0.703 mol A- in 130.1 mL  after 0.158 g of NaOH was added? [Ka= 1.56 ×10-5] Report your answer with three decimals. Enter numbers only; do not enter units.

Which of the following mixtures would result in a buffer solution when 1.0 L of the two solutions are mixed? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a 0.2 M HNO3 and 0.4 M NaNO3 b 0.2 M HNO3 and 0.4 M HF 0.2 M HNO3 and 0.4 M NaF d. 0.2 M HNO3 and 0.4 M NaOH e None of the above would result in a buffer solution.

A 50.0-ml sample of 0.20 M hydrochloric acid (HCI) is titrated with 0.5 M LIOH. Determine the pH of the solution after the following volumes of LIOH titrant are added. Express your answers to two decimal places. a) pH after 10 mL of LIOH added: b) pH after 20 mL of LIOH added: c) pH after 30 mL of LIOH added: Check

Calculate the pH for each case in the titration of 50.0 mL of 0.220 M HCIO(aq) with 0.220 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 40.0 mL KOH? pH =

7. A solution was made by mixing 50.0 mL of 0.750 M HCN with 25.0 mL of water. What is the pH of this solution? The pka of HCN = 9.31. 8. One of the compounds featured on the TV series "Breaking Bad" was hydrofluoric acid (HF), pKa = 3.14. a) A solution of HF has a pH = 1.77. What was the initial [HF] for this solution in mol L-1? b) What is the equilibrium concentration of F in this solution in mol L-1? c) What is the percent ionization of HF in this solution?

A student wants to make a 0.75 mol/L buffer solution using potassium hydrogen sulfate, KHSO4, and a conjugate base. Which of the following options could be used as a conjugate base to make this buffer solution? Answer choices a 0.80 mol/L solution of H2SO4 a 0.50 mol/L solution of K2SO4 a 0.002 mol/L solution of K2SO4 a 9.0 mol/L solution of KHSO4

Please answer

Determine the resulting pH when 0.040 mol of solid NaOH is added to a 200.0 mL buffer containing 0.100 mol C6H5NH3CI and 0.500 M C6H5NH2. The value of Kb for C6H5NH2 is 4.3 x 101°. 1 2 3 4 NEXT Use the table below to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of liquid water in the reaction. C6H;NH3*(aq) Он (aq) H20(1) C6H;NH2(aq) + + Before (mol) Change (mol) After (mol) 5 RESET 0.040 -0.040 0.500 -0.500 0.100 -0.100 +x 0.040 + x 0.040 - x 0.100 + x 0.100 - x 0.060 -0.060 -x 0.140 -0.140 0.020 -0.020

Calculate the pH for each case in the titration of 50.0 mL of 0.140 M HCIO(aq) with 0.140 M KOH(aq). Use the ionization constant for HC1O. 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