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- A volume of 50 mL of 1.8 M NH3 is mixed with an equal volume of a solution containing 0.95 g of MgCl2. What mass of NH4Cl must be added to the resulting solution to prevent the precipitation of Mg(OH)2?In a titration of cyanide ion, 28.72 mL of 0.0100 M AgNO3 is added before precipitation begins. [The reaction of Ag+ with CN- goes to completion, producing the Ag(CN)2- complex. Precipitation of solid AgCN takes place when excess Ag+ is added to the solution, above the amount needed to complete the formation of Ag(CN)2-. How many grams of NaCN were in the original sample?5) 3 L contaminated air 50 mL 0.0116 M in an air pollution analysis Carbon dioxide (CO2) BaCO3 is passed through Ba (OH) 2 solution. as precipitated. Excess of base, next to phenol phthalate (f.f.) indicator It is titrated with 23.6 mL of 0.0108 M HCl. CO2 in this air sample Calculate its concentration in ppm. (Density of CO2 Take it as 1.98 g / L. C = 12, O = 16 g / mol).
- A chemistry graduate student Is given 500. mL of a 1.60M propanolc acdd (HC,H.CO,) solution. Propanoic acid is a weak acid with K=1.3x 10 -5 What mass of KC,H.CO, should the student dissolve in the HOC,H.CO, solution to turn it into a buffer with pH =4.537 D. 2. You may assume that the volume of the solution doesn't change when the KC,H.CO, is dissolved in it. Be sure your answer has a unit symbol, and round It to Ar 21 2 significant digits. x10 Explanation Recheck © 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Accessibility V O 8:43 hp esc -> & 大 ! #3 backs 6. 9 1 3. W r y [ 1 tab + |/ * 00 %243.2. Calculate the mass of NH.CI that should be dissolved in 525.00 mL. of 0.1531 M NH3 (Ko = 1.8 x 10-5) solution to prepare a buffer with a pH of 10.00. Assume that the change in volume on addition of NH.Cl is negligible.3 L contaminated air 50 mL 0.0116 M in an air pollution analysisCarbon dioxide (CO2) BaCO3 is passed through Ba (OH) 2 solution.is precipitated as. Excess of base, next to phenol phthalate (f.f.) indicatorIt is titrated with 23.6 mL of 0.0108 M HCl. CO2 in this air sampleCalculate its concentration in ppm. (Density of CO2Take it as 1.98 g / L. C = 12, O = 16 g / mol).
- In which case will a precipitate form? (i) a 0.050 M MnCl2 solution with pH = 8.00 (Does Mn(OH)2 precipitate?) Ksp = 1.9 x 10-13. (ii) 100. mL of 0.010 M AgNO3 is added to 20. mL of .050 M Na2SO4 (Does Ag2SO4 precipitate?) Ksp = 1.4 x 10-5.If 20.0 mL of 0.50M NH3 is added to 80.0 mL of 0.0010M FESO4 and then enough NHẠC1 is added so that the NH4* present becomes 1.0M, a) What will be the [OH-] in the resulting solution? b) Will Fe(OH)2 precipitate? %3D K½ for ammonia = 1.8 x 10-5; Ksp for Fe(OH)2 = 1.6 x 10-143 L contaminated air 50 mL 0.0116 M in an air pollution analysisCarbon dioxide (CO2) is precipitated as BaCO3 by passing through Ba (OH) 2 solution. The excess of the base is titrated with 23.6 mL 0.0108 M HCl in addition to the phenol phthalate (f.f.) indicator. Calculate the CO2 concentration in this air sample in ppm. (Take the density of CO2 as 1.98 g / L. C = 12, O = 16 g / mol).
- 5.) A 4.59mL sample of HCl (sp. gr. = 1.3) required 5.5mL of 0.9544N NaOH in titration. Calculate the %w/w of HCl in the sample.A chemistry graduate student is given 250. mL of a 1.10 M trimethylamine ((CH;),N) s solution. Trimethylamine is a weak base with K;= 7.4 x 10 '. What (CH3), NHBr should the student dissolve in the (CH;),N solution to turn it into a buffer with pH = 11.41? mass of You may assume that the volume of the solution doesn't change when the (CH, NHBR is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.A 0.4755-g sample containing (NH,),C,O, and inert materials was dissolved in water and 3. strongly alkaline with KOH, which converted NH,* to NH3. The liberated NH; was distilled into 50.0mL of 0.05035 M H,SO The excess H,SO, was back titrated with 11.13 mL of 0.1214 M NaOH. Calculate the following: A. The % N (14.00 g/mole) B. The % (NH,),C,0;(124.10 g/mole) in the sample