4) How would your calculated value of Ksn be affected by errors introduced from the following sources? Be specific in your answer. State whether Ksp Would be too large, too small, or not affected, and explain why that error would have that effect on Kep- The precipitate of Ca(IO3)2, when obtained originally, is not washed with distilled water. b The Na2S2O3 was not standardized, so its nominal molarity was used instead of a standardized molarity. Note that Na2S203 solutions can air oxidize over time. Although the KIO3 used to standardize the Na2S203 is labeled as 0.0100 M, its actual concentration is somewhat higher than 0.0100 M. Extraneous water is introduced from wet filter paper or wet funnels, or by washing the precipitate during the final filtration of Ca(IO3)2.

4) How would your calculated value of Ksn be affected by errors introduced from the following sources? Be specific in your answer. State whether Ksp Would be too large, too small, or not affected, and explain why that error would have that effect on Kep- The precipitate of Ca(IO3)2, when obtained originally, is not washed with distilled water. b The Na2S2O3 was not standardized, so its nominal molarity was used instead of a standardized molarity. Note that Na2S203 solutions can air oxidize over time. Although the KIO3 used to standardize the Na2S203 is labeled as 0.0100 M, its actual concentration is somewhat higher than 0.0100 M. Extraneous water is introduced from wet filter paper or wet funnels, or by washing the precipitate during the final filtration of Ca(IO3)2.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Hw.128.
Determine the molar solubility for Ag2SO4 (Ksp= 1.5 x 10-5) in a solution that already contains 0.200 M AgNO3.
Please don't provide handwritten solution
A 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.
Can you show the calculations step by step? Where did 3.1e-5 came from
Consider a scenario wherein a mixture containing 4.23 x 10-3 M Sr2+ and 1.12 x 10-4 M F was prepared. SrF₂(aq) = Sr²+ (aq) + 2F (aq) A. What is the Qsp of the mixture? [Select B. In the given scenario, will a precipitate (K-2.5 × 10%) form? [Select]
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). What is the identify of the solid species? Write out the balanced equation for the solubility of the insoluble solid. Uses physical state symbols, an equal sign instead of a reaction arrow, and spaces where necessary. Example: (AgCl(s) = Ag+(aq) + Cl-(aq)) What is the value of the Qsp? Give your answer in exponential form and to three sig. figs. (e. g. 1.23E-3). THIS IS PART 1 WILL POST OTHER QUESTIONS AS PART 2
At 15 ° C and in pure water, the solubility of AgCl (silver chloride) is 8.4×10−5 mol.L-¹. The one of silver bromide (AgBr) is 3.8×10-7 mol.L-¹. What are their solubilities in a solution saturated by both the salts? The answer : s(AgCl) = 8.4×10−5 mol.L=1; s(AgBr) = 1.7×10-9 mol.L
The molar solubility of Ba(1O3)2 in a solution that is 0.0600 M in Ba(NO3)2 at 25°C is: (Ksp = 1.57 x109) M 10-4 x 1.40 .a O M 103 x 4.27 .b o M 106 x 6.40.c M 10-5 x 8.09.d M 104 x 2.79 .e O
Consider the following mixtures of chemicals. Complete the table by writing balanced equations and calculating the value of Q. Hence indicate whethe precipitation will occur. Mixture Balanced equation Ksp Q Precipitation occurs (yes or no) 100mL 0.5 molL-1 Ca(NO3)2 mixed with 100 mL 0.2 molL-1 Na2SO4 20 mL 0.01 molL-1 AgNO3 mixed with 80 mL 0.05 molL-1 K2CrO4
Suggest a strategy using selective precipitation (which salts containing precipitating ion would you add and in what order) to purify wastewater contaminated with Ag+, Ba2+, Fe3+ and Na+. The purified water should only contain Na+ which is safe to drink.
What happens when equal volumes of 4x10-4 M aqueous solutions of calcium nitrate, Ca(NO3)2, and sodium fluoride, NaF, are combined? The Ksp of calcium fluoride, CAF2, is 4.0×10-11 Periodic Table and Datasheet O Q K; no precipitate forms O Q K; a precipitate forms