7. Consider a buffered solution at a pH of 4.00 made with HF (K₁ = 7.2 x 104) and NaF. Which of the following statements is true? Assume all of the concentrations below refer to equilibrium concentrations. A) [HF] = [F] B) [HF] = [H*] C) [HF] > [F] D. [H] = [F] E. [HF] [F]

Which weak acid would be best to use when preparing a buffer solution with a pH of 6.2? An acid with K, = 2.5 x 10-3 An acid with K, = 3.2 x 10-7 An acid with K, = 2.5 x 10* An acid with K, = 1.7 x 10-10 An acid with K, = 1.0 x 10-"

100.0 mL of HCI required 25.00 mL of 0.2000 M Mg(OH)2 to reach pH 7. What is the concentration of the HCI ? 2 HCI + Mg(OH)₂ MgCl₂ + 2 H₂O The neutralization equation is There is enough information to calculate the moles of Mg(OH)2 ( L Mg(OH)₂ (- concentration = Then use stoichiometry to convert moles of Mg(OH)₂ into moles of HCI mol HCI a. acid i. 0.2000 p. 0.01000 mol Mg(OH)₂ (- b. base c. HCI d. NaOH mol Mg(OH)2 We now can calculate the concentration of HCI since we have both the moles of HCI and the volume of HCI j. 1.000 k. 0.005000 q. 0.001000 1 L mol HCI LHCI r. 58.31 = mol Mg(OH)2 e. NaCl I. 100.0 f. H₂O m. 0.1000 s. 5.831 = g. 25.00 mol/L n. 0.05000 h. 0.02500 mol Mg(OH)2 o. 2.000 mol HCI

by the addition of strong base in a buffer, pH of the solution is maintained by?  1- Shifting equilibrium toward right side  2- Shifting equilibrium toward left side  3- by producing weak acid and more H ions  4- by producing conjugate base and more OH ions

Determine the molar concentrations of Ca2+ and CI- in a 0.38 M calcium chloride solution. 1) 0.38 M Ca2+ and 0.38 M CI- O 2) 00.19 M Ca2+ and 0.38 M CI- 3) 0.38 M Ca2+ and 0.76 M CI- 4) 0.19 M Ca2+ and 0.76 M CI- O 5) None of the above

Need help with question number one

I. Consider a 1.00 L of 1.50x10^-3 M hydrocyanic acid (HCN, K=4.9×10^-10) 1. Write the equilibrium expression. 2. Calculate the pH of the solution. 3. If a 9.00x10^-4 mol sodium cyanide, NaCN, is added, what is the pH of the resulting solution? Assume negligible volume change.

Please help with this question  a)Which of the following mixtures may be act as a buffer solution? HBr, NaBrHBr, NaBr HCl, NaClHCl, NaCl HI, NaIHI, NaI HF, NaFHF, NaF b) Which solution will have the highest pH? The Ka of HClO is 3.8x 10-8 M   A solution of 100 mL of water with 20 mL of 0.1 M NaOH added.   A 100 mL buffer solution of 0.1 M HClO, 0.1 M ClO? with 20 mL of 0.1 M NaOH solution added.   A buffer solution of 0.1 M HClO, 0.1 M ClO?.   A 100 mL buffer solution of 0.1 M HClO, 0.1 MClO? with 20 mL of 0.1 M HCl solution added. c)What is the pH of 100 mL100 mL of a buffer that is 0.5 M HCNO0.5 M HCNO and 0.5 M CNO−0.5 M CNO− when 100 mL100 mL of a 0.2 M NaOH0.2 M NaOH solution is added? Assume the volumes are additive. KaKa of HCNO is 3.5 × 10−4

Macmillan Learning Select the statements that describe a method which can be used to make a buffer. Partially neutralize a strong acid solution by addition of a strong base. Add appropriate quantities of weak acid and its conjugate base to water. Partially neutralize a weak base solution by addition of a strong acid. Partially neutralize a strong base solution by addition of a strong acid. Partially neutralize a weak acid solution by addition of a strong base. OCT 12 3o) N A

Name Formula Ka Acetic Acid CH3COOH 1.8x10^-5 Chloroacetic acid C2H3ClO2 1.3x10^-3 Formic Acid HCOOH 1.7x10^-4       Consider a buffer solution consisting of CH3COOH and CH3COONa with a pH of 4.9 Select the true statement about this buffer solution. A. [CH3COOH] <[CH3COONa]  B. [CH3COOH]= [CH3COONa] C. [CH3COOH]> [CH3COONa]