Consider the following reaction: CH,COOH(aq) + Of (ag) - CH,COO (ag) + H,0(1) 2nd attempt Jl See Perlodic Table How much 5.70 MNAOH must be added to 540.0 mL of a buffer that is 0.0180 Macetic acid and 0.0250 M sodium acetate to raise the pH to 5.75? ml.
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- 10. 50 cm3 of 0.05 M weak acid solution is titrated with 0.1 M NaOH solution. The measured pH valuesare 7.345 and 7.497 at the consumptions of 6.0 and 6.1 cm3, respectively. What value of the buffer capacity can be calculated in the solution at pH = 7.421?11. Based on the data given in question 10, what is the total concentration of the anion of the weak acid atthe given point?If 0.3074 g of a mixture of pure KCl and KBr requires 30.98 mL of 0.1007 M AgNO3 solution for its titration, calculate the% KCl and KBr in the sample. (Pat Data: Cl, 35.453; Br, 79.904; K, 39.098)what 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
- The solubility of Ag2CrO4 (Ksp = 1.2 x 10-12) is several times greater than that of AgCl (Ksp = 1.82 x 10-10), so the red precipitate cannot form until all the chloride ions have effectively been removed from the solution. If a student uses 1 mg of K2CrO4 Aas an indicator for 100 mL of sample solution, what is the concnetrion of chloride ion in the solution when the red precipitate (Ag2CrO4) starts to form?A 50-mL solution of 0.5005 N standard NaOH was added to a 0.9250-g sample of Aspirin and was boiled for 10 minutes. After cooling a full pipet of phenolphthalein was added to the solution before it was titrated with 24.7 mL of 0.5015 N standard HCl solution until the disappearance of the pink color. The same procedure was carried using a blank which consumed 4.6 mL of the same standard acid. Calculate for the %Aspirin in the sample. Atom weights: C =12, H =1, O =16.Calculate the pH of a mixture containing 50 mL of 0.1 M NaH2PO4 and 150 mL of 0.1 MNa2HPO4. How many mL of 0.1 M H3PO4 should be added to the above buffer to lower thepH to 7.0? Would the resulting solution be of higher or lower ionic strength than the original200 mL buffer solution? Explain.
- 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.Unlike propanoic acid, magnesium hydroxide, Mg(OH)2 does not dissolve well in water. The Ksp of Mg(OH)2 is only about 2 × 10–11. Yet, what will be the result if 75 mL of 0.0050 M Mg2+ are mixed together with 55 mL of 0.00010 M OH–? Write an appropriate expression (equation) for the Ksp of Mg(OH)2(s). Then, calculate Qsp and state accordingly whether a precipitate will form or notThe value of ?? for the reaction: AgBr (s) ⇋ Ag+(aq) + Br−(aq)It is 7.7 × 10−13 at 25 ° C. Determine the solubility of AgBr in:a) Distilled H2O.b) A 0.01 M solution in CaCl2
- (a) For the precipitation reaction: A+ + B– AB(s)Calculate the value of the equilibrium constant for 99.99% conversion to AB atthe equivalence point, assuming that the analyte content is 5.00 mmole and thetotal volume at the equivalence point is 100.00 mL.(b) What factors affect end-point sharpness in a precipitation titration? Explain.(c) Explain briefly why silver nitrate is an important reagent used in precipitationtitrations.(d) Mohr Method, Volhard Method and Fajans Method are commonly used for thevolumetric analysis of chlorides. Distinguish the three methods in terms of thetitrants and indicators used, and how the titrations are carried out.A buffer is made from 25.0mL of 1.0M CH3COOH and 25.0mL of 1.0M CH3COONa, what would be the pH of the buffer?Calculate the solubility at 25°C of AgBr in pure water and in 0.49M NaCN. You'll probably find some useful data in the ALEKS Data resource. Round your answer to 2 significant digits.