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- 4. a) Data in the following table are obtained for the titration of 0.297g sample of a solid, monoprotic weak acid with a 0.150M NaOH solution. Plot PH vs. V.Determine the molar solubility (?) of Ag2CO3 in a buffered solution with a pH of 5.887 using the systematic treatment of equilibrium. ?sp(Ag2CO3) = 8.46×10−12; ?a1(H2CO3) = 4.45×10−7; ?a2(H2CO3) = 4.69×10−11. S = ? MA buffer is prepared by mixing 0.15 M Na HPO4 and 0.10 M NaH, PO4. Kg for H3PO4 = 7.5 103 K, for H,PO, = 6.2 x 10 8 K, for HPO,2- = 4.2 x 10°13 1) What is the pH of this buffer? 2) Write the chemical reaction that occurs when NaOH is added to this buffer.
- A saturated solution of Pb(OH)2 is filtered and 25.00 mL of this solution is titrated with 0.000050 M HCl at 25°C. The volume required to reach the equivalence point of this solution is 6.70 mL. Calculate the concentration of OH", Pb2* and the Ksp of this saturated solution.Please don't provide hnad writtin solution.....A buffer is made up of equal volumes of 0.1 M weak acid (AH) and 0.1 M conjugate base (A minus). The pH of the solution is measured to be 4.6. What is the pk, of this weak acid? (HINT: Use the formula pH = pK, + log(Vol A minus/ Vol HA)) %3D O 2.6 O 1.6 O 5.6 O 3.6 O 4.6
- A chemistry graduate student is given 450. mL of a 1.80M chlorous acid (HCIO,) solution. Chlorous acid is a weak acid with K= 1.1 × 10 . What mass of KC1O, should the student dissolve in the HC1O, solution to turn it into a buffer with pH = 1.92? You may assume that the volume of the solution doesn't change when the KCIO, is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.A butanoic acid/potassium butanoate (C,H,COOH/KOOCC,H,) buffer is prepared to 1.12x10-2 mol L1CH,COOH and 8.38x10-3 mol L1 KOocC;H. The K, for butanoic acid is 1.5x10-5. What is the pH of the buffer solution? Part A O 4.82 O 4.70 O 5.25 O 4.65 O 4.95 o o o o owhat is the pH of a buffer made from 0.350 mol of HBrO (ka = 2.5 * 10^-9) and 0.120 mol of KBrO in a 2.0 L of solution? go into as much detail as possible please
- • A mixture is prepared by combining 3.0 mL of 0.0050 M NaSCN (in 0.10 M HNO3) solution with 4.0 mL of 0.0030 M Fe(NO3)3 solution, and 3.0 mL of 0.10 M HNO3 solution. Based on your average Kf value, determine the equilibrium concentrations of Fe 3+, SCN, and FeSCN2+ in the solution. You cannot apply a small x approximation.A pipette is used to add 41 mL of 0.2 M Pb(NO3)2 to a 268.0 mL solution of 0.2 M NaF. Determine the equilibrium concentration of Pb2+(aq) in the final solution. Ksp(PbF2)=3.6E-8Include at least 3 significant figures in your answer.A chemistry graduate student is given 100. mL of a 0.40M nitrous acid (HNO,) solution. Nitrous acid is a weak acid with K 4.5 x 10. What mass of -4 NaNO, should the student dissolve in the HNO, solution to turn it into a buffer with pH =3.16? %3D You may assume that the volume of the solution doesn't change when the NaNO, is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. x10 Submit Assignment Continue 2021 McGraw Hill LLC. AlI Rights Reserved. Terms of Use Privacy Center | Accessibility MacBook Air F11 Fig