+2, and 4.03. the following 0.10 M solutions available: CH3COOH, NACH:C00, NHẠCI, NH3, NAHCO:, and Na2CO3. Which solution(s) will you choose to design each buffer? pH 4.56 pH 9.10 pH 10.45

Calculate the volume of TAE buffer that you will need to prepare a 100ml solution of 1X strength if you only have a 50X concentrated solution available.

Which of the following combinations would be the best choice to buffer the pH of a solution at approximately 7? Ionization Constants for Aqueous Weak Acids at 25 °C Acid K. (pK,) Conjugate Base Hydrogen phthalate ion, Cg H4(CO2H)(CO2) Acetic acid, CH3 CO,H Acetate ion, CH; CO2- 1.8 x 10-5 (4.74) Weak Acid Phthalic acid, C6 H4 (CO,H)2 1.3 x 10-3 (2.89) Dihydrogen phosphate Hydrogen phosphate ion, H2 PO4 Hydrogen phosphate ion, HPO42 6.2 x 10-8 (7.21) ion, HPO,2- Phosphate ion, PO,* 3.6 x 10-13 (12.44) O Na, HPO4 and NagPO4 O NaH2 PO4 and NazHPO4 O H;PO4 and NaH2 PO4

A base is added to a 0.050 M solution of MnCl2, raising the pH gradually. Calculate the pH of the solution when 88 of the manganese has precipitated? Table 5-7 Solubility-Product Constants, K, at 25°C Fluorides Chromates (cont.) Ag, Cro, PbCro, Hydroxides (cont) Ni(OH), Zn(OH), Cu(OH), Hg(OH), Sn(OH), Cr(OH), A(OH), BaF, MgF, PbF, SrF, CaF, 2.4 x 10-5 X 10-8 x 10-8 1.9 x 10-12 1.6 x 10-16 4.5 X 10-17 1.6 x 10-19 3 2 x 10-16 4 Carbonates 7.9 x 10-10 3.9 x 10-11 X 10-26 NiCO, CaCO, BaCo, SrCO, CuCO, ZnCO, MnCO, 1.4 x 10-7 3 10-27 4.7 x 10- 6.7 x 5 x 6 x 10-38 2.5 x 10-43 Chlorides 10-31 1.6 x 10- 1.7 x 10-10 1.1 x 10-18 1.6 x 10-9 7 x 10-10 2.5 x 10-10 10-33 PBCI, AgCi Hg,Cl, Fe(OH), Co(OH), Sulfides 2 x 10-10 8.8 x 10-11 2.1 x 10-11 Bromides X 10-16 X 10-19 3 x 10-21 X 10-22 2.5 x 10-22 X 10-26 1.0 x 10-28 MnS 7. PbBr, AgBr Hg, Br, 4.6 x 10-6 5.0 x 10-13 Feco Ag,CO, CdCo, PBCO, MgCO, Hg,CO, Fes 4 8.2 x 10-12 5.2 x 10-12 1.5 x 10-15 1 x 10-15 NiS 1.3 x 10-22 Cos ZnS lodides Pbl, Agl…