Elc. A JU student was asked to prepare a pH = 4.0 acid solution in which the molarity of H is 1.0 x 10-4 M. The only acid that is available is sulfuric acid, H2SO4. Assume that H2SO4 (1) will completely dissociate according to Eq. 1. H2SO4 (aq) S0 (aq)+2H* (aq) First, the student transferred 1.500 mL pure H2SO4 into a volumetric flask and made 200.0 mL solution (solution 1). The density of pure H2SO4 is 1.84 g/mL. Then he transferred exactly 10.00 mL solution 1 with a pipet into another volumetric flask and made 250.0 mL solution (solution 2). Please calculate the molarities of both solutions for him. If he can solve this problem correctly, it will prove to his supervisor he has necessary skills.

Calculate the pOH of a 0.0376 M HCIO solution at each temperature. 0°C pOH = 35 °C pOH = T (°C) 0 5 10 15 20 30 35 40 45 50 100 Kw 1.15 x 10 1.88 x 10 2.97 x 10 4.57 x 10 6.88 x 10 1.46 × 10 2.07 x 10 2.88 x 10 3.94 x 10 5.31 x 10 5.43 x 10 45 45 44 H 45 15 15 14 +4 44

At 25 °C, only 0.0110 mol of the generic salt AB2 is soluble in 1.00 L of water. What is the Ksp of the salt at 25 °C? AB, (s) = A2+(aq) + 2B¯(aq)

The calculated concentration of Ag+(aq) from the student’s data is lower than the actual concentration of the original solution. The student claims that the calculated concentration is too low because some of the AgCl(s) passed through the filter paper. Do you agree or disagree? Justify your answer.

Sagar

Metal sulfides are prepared by bubbling hydrogen sulfide gas, H2S, through an aqueous solution containing the metal ion, and then adjusting the pH. When the solution is saturated with H2S, which occurs when [H2S]=0.100 M, the equilibrium shown is established.   H2S(aq)+2H2O(l)↽−−⇀S2−(aq)+2H3O+(aq)?eq=1.1×10−20 An aqueous solution containing 0.0570 M Pb2+ and 0.0570 M Ag+ is saturated with H2S. Above what concentration of S2− will PbS precipitate? The ?sp of PbS is 8.9×10−29. [S2−]=   M Above what concentration of S2− will Ag2S precipitate? The ?sp of Ag2S is 3.3×10−50. [S2−]=   M If the pH of the solution is adjusted to 2.83, which species will precipitate from the saturated H2S solution? both PbS and Ag2S neither species PbS Ag2S

Give detailed Solution

You are asked to test the electrolyte performance of several aqueous solutions. Based on the trends of solubility and dissociation, rank the following solutions from strongest to weakest electrolyte: 1 M Na₂SO4 (aq) 1 M HCOOH (aq) (Formic acid) CH3CH₂OH (1) H₂O(l) 1 M HCI (aq) Na2SO4 > HCOOH > HCI > H2O > CH3CH2OH Na₂SO4 > HCI > HCOOH > H2O > CH3CH2OH | Na2SO4 > HCOOH > CH3CH2OH > H2O > HCI HCI > HCOOH > Na2SO4 > H2O > CH3CH2OH | H2O > CH3CH2OH > Na2SO4 > HCOOH > HCI

Consider an amphoteric hydroxide, M(OH)2(s) , where M is a generic metal. M(OH)2(s)↽−−⇀M2+(aq)+2OH−(aq)?sp=6×10−16 M(OH)2(s)+2OH−(aq)↽−−⇀[M(OH)4]2−(aq)?f=0.06 Estimate the solubility of M(OH)2 in a solution buffered at pH = 7.0, 10.0, and 14.0.   solubility at pH = 7.0 M   solubility at pH = 10.0 M   solubility at pH = 14.0 M

Part A) A 10.0 mL sample of 0.250 mol/L NiF2(aq) is mixed with 20.0 mL of 0.0900 mol/L NaOH(aq) and then diluted to a final volume of 100. mL.Calculate the concentration of Ni2+ ions in the 100 mL mixture before the reaction starts. Express your answer to three significant figures.ksp: 5.48e-16