A 190.0 mL solution of 2.765 M strontium nitrate is mixed with 215.0 mL of a 3.581 M sodium fluoride solution. Calculate the mass of the resulting strontium fluoride precipitate. 48.30 mass: g Assuming complete precipitation, calculate the final concentration of each ion. If the ion is no longer in solution, enter a 0 for the concentration. 3.576 [Na*] =| M Incorrect 2.763 [NO,] = M Incorrect 0.739 [Sr*] = M Incorrect 1.788 [F=] = M Incorrect
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![A 190.0 mL solution of 2.765 M strontium nitrate is mixed with 215.0 mL of a 3.581 M sodium fluoride solution. Calculate the
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mass of the resulting strontium fluoride precipitate.
The sodium ion concentration you
calculated is incorrect.
When calculating the Na+
concentration, you may have used the
48.30
mass:
volume of the original NaF solution.
Instead, use the total volume of both
Assuming complete precipitation, calculate the final concentration of each ion. If the ion is no longer in solution, enter a 0 for
solutions to calculate the concentration
the concentration.
in the final solution.
3.576
[Na*] =
M
Incorrect
2.763
[NO,] =
M
Incorrect
0.739
[Sr**] =
M
Incorrect
1.788
[F=] =
M
Incorrect](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4cbada35-3122-4a6c-a25c-246bca0ae236%2F74d42509-6a39-4c94-bfeb-599449db7f5b%2Fsb6mzks_processed.png&w=3840&q=75)
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- 1ml of 1mg/ml of diluted aspirin powder solution is titrated by 0.005M NaOH. Before titration, 5 ml ethanol, 14 ml CO2 free water, and 4 drops bromothymol blue indicator is added into diluted aspirin powder solution. Mass of 0.005M NaOH used is obtained by weight titration = 1.1384g . [Molar mass of aspirin =180.15]; for solution, 1g=1mL at 25 degree Celcius. Calculate the purity of the powder.A commercial vinegar was analyzed by titration to determine the percent acetic acid. Briefly, 10.00 mL of vinegar sample was diluted to 100. mL solution in a volumetric flask. A 25.00 mL aliquot from the diluted vinegar required 25.55 mL of 0.1005 M sodium hydroxide to reach the phenolphthalein endpoint From this experiment which is the standard solution used in titration? CH3COOH NaOH NaCH3COO C20H14O4A solution is prepared by mixing 20.0 mL of 0.100M Fe(NO3)3 with 20.0 mL of 0.00300M KSCN and 10.0 mL of DI water. Calculate the initial concentration of Fe^3+ in this solution? Give answer with correct amount of sig figs.
- Ammonium acetate buffer is used as an important reagent for studying molecular biology, biological buffers, reagents and DNA and RNA purification. Ammonium acetate (0.24M) in combination with cold 66% (v/v) ethanol quantitatively precipitated RNA from very dilute solutions (greater than or equal to μg/ml) after centrifugation. Ammonium acetate (CH3COONH4) is also a salt of weak acid (CH3COOH) and weak base (NH4OH). The Ka and Kb are equal to 1.8 x10-5. The pH of this salt solution will be, a. pH > 7 b. pH ≈ 7 c. pH < 7 d. both cation and anion don’t hydrolyze. e. none of the above.A BS Medical Technology student was asked to determine the molecular weight of a diprotic acid using acid-base titration. This student performed fourtrials. Firstly, the student used potassium hydrogen phthalate (KHP, 204.22 g/mol) as standard to determine the exact concentration of the NaOHtitrant. The results of the student are summarized in the table below:Note: The stoichiometric relationship of KHP to NaOH is 1:1Standardization Trial 1 Trial 2 Trial 3 Trial 4KHP Mass, g 0.5033 0.5066 0.6989 0.6843Volume NaOH used, mL 24.32 25.61 24.67 24.56After the standardization, the student weighed different amounts of the unknown acid. In a similar fashion, the student performed acid-base titrationusing phenolphthalein as indicator. The results of the molecular weight determination are summarized below:Note: The stoichiometric relationship of Unknown acid to NaOH is 1:2Molecular WeightDeterminationTrial 1 Trial 2 Trial 3 Trial 4Unknown Mass, g 0.1234 0.1034 0.1178 0.1322Volume NaOH used, mL…A BS Medical Technology student was asked to determine the molecular weight of a diprotic acid using acid-base titration. This student performed fourtrials. Firstly, the student used potassium hydrogen phthalate (KHP, 204.22 g/mol) as standard to determine the exact concentration of the NaOHtitrant. The results of the student are summarized in the table below:Note: The stoichiometric relationship of KHP to NaOH is 1:1Standardization Trial 1 Trial 2 Trial 3 Trial 4KHP Mass, g 0.5033 0.5066 0.6989 0.6843Volume NaOH used, mL 24.32 25.61 24.67 24.56After the standardization, the student weighed different amounts of the unknown acid. In a similar fashion, the student performed acid-base titrationusing phenolphthalein as indicator. The results of the molecular weight determination are summarized below:Note: The stoichiometric relationship of Unknown acid to NaOH is 1:2Molecular WeightDeterminationTrial 1 Trial 2 Trial 3 Trial 4Unknown Mass, g 0.1234 0.1034 0.1178 0.1322Volume NaOH used, mL…
- A BS Medical Technology student was asked to determine the molecular weight of a diprotic acid using acid-base titration. This student performed fourtrials. Firstly, the student used potassium hydrogen phthalate (KHP, 204.22 g/mol) as standard to determine the exact concentration of the NaOHtitrant. The results of the student are summarized in the table below:Note: The stoichiometric relationship of KHP to NaOH is 1:1Standardization Trial 1 Trial 2 Trial 3 Trial 4KHP Mass, g 0.5033 0.5066 0.6989 0.6843Volume NaOH used, mL 24.32 25.61 24.67 24.56After the standardization, the student weighed different amounts of the unknown acid. In a similar fashion, the student performed acid-base titrationusing phenolphthalein as indicator. The results of the molecular weight determination are summarized below:Note: The stoichiometric relationship of Unknown acid to NaOH is 1:2Molecular WeightDeterminationTrial 1 Trial 2 Trial 3 Trial 4Unknown Mass, g 0.1234 0.1034 0.1178 0.1322Volume NaOH used, mL…How would you use an experimentally determined Ksp value to calculate that Ag2CrO4 should precipitate when 5ml of 0.0040 M AgNO3 are added to 5ml of 0.0024 M K2CrO4. You can come up with your own experimentally Ksp value. I just want to see steps in solvingA sample solution contains two unknown ions. A student did a series of tests on the solution, in the order listed below. If a precipitate formed at any stage, the mixture was filtered and further tests were done on the filtrate. The results are as follows. First test:Second test:Third test:Fourth test: solution is a pink colourNaIO3(aq) added and no precipitate formsflame colour is redNa2CO3(aq) is added and no precipitate forms Two possible ions that the solution contains are a.lithium and manganese(II) b. strontium and cobalt(II) c. strontium and manganese(II) d. lithium and cobalt(II)
- Calculate the Qsp or Ksp, as indicated, and determine whether a precipitate will form when each of the following mixtures is prepared. (You may assume temperature is held constant, volumes are additive, and that the initial solutions, prior to mixing, are unsaturated.) (a) 25.15 mL 1.51 ✕ 10−4 M CaCl2 is mixed with 25.31 mL 3.20 ✕ 10−3 M NaF. (Ksp for CaF2 = 3.5 ✕ 10−11) Qsp A precipitate will form. A precipitate will not form. (b) 14.86 mL 3.50 ✕ 10−3 M Pb(NO3)2 is mixed with 34.80 mL 1.78 ✕ 10−4 M Na2SO4. (Ksp for PbSO4 = 2.5 ✕ 10−8) Qsp A precipitate will form. A precipitate will not form.PART 2: A solution is prepared by mixing 150.0 mL of 0.0010 M magnesium nitrate and 250.0 mL of 0.100 M sodium fluoride (Ksp = 7.4x10-11). Is Ksp greater than , equal to, or lower than Qsp? Will a precipitate form, Y/N? What is the fluoride ion concentration (in solution) after mixing is complete? Give your answer in exponential form and to three sig. figs. (e. g. 1.23E-3). What is the magnesium ion concentration (in solution) after mixing is complete? Give your answer in exponential form and to three sig. figs. (e. g. 1.23E-3).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 not