Calculate the molar solubility of Fe(OH)3 (Ksp = 4.0 x 10-38) in each of the following solvents. Enter your answer, rounded to the correct number of significant figures, into the answer box using scientific notation using the E notation. a) pure water solubility= 4.0E-17 M b) a solution buffered to pH = 5.00 solubility = 4.0E-11 M c) a solution buffered to 11.00 solubility = 4.0E-29 M

The weak monoprotic acid, acetic acid, is titrated with the strong base, potassium hydroxide as follows: HC2H3O2(aq) + K+ OH- (aq) → K+ C2H3O2-(aq) + H2O(l) Ka for acetic acid is 1.81 x 10-5 (at 25 oC). A 25.00 mL sample of a solution of acetic acid with concentration 0.0833 M is titrated with 0.1000 M KOH. 1. what is the pH when the volume of base added equals half the volume of the equivalence point? 2. what is the pH of the titration when 20.00 mL of base have been added? 3. what is the pH of the titration when 30.00 mL of base have been added?

The weak monoprotic acid, acetic acid, is titrated with the strong base, potassium hydroxide as follows: HC2H3O2(aq) + K+ OH- (aq) → K+ C2H3O2-(aq) + H2O(l) Ka for acetic acid is 1.81 x 10-5 (at 25 oC). A 25.00 mL sample of a solution of acetic acid with concentration 0.0833 M is titrated with 0.1000 M KOH. a) Sketch the pH vs volume of added base titration curve for this reaction. pH vertically, volume of base horizontally. Label your axes with correct pH and volumes. (Attach more space, if needed) b) what is the pH at the beginning of the titration, Vbase = 0.00 mL ? c) what is the volume of the base needed to reach the equivalence point ? (label the equiv. point) d) what is the pH at the equivalence point?e) what is the pH of the titration when 5.00 mL of base have been added ? f) what is the pH when the volume of base added equals half the volume of the equivalence point? g) what is the pH of the titration when 20.00 mL of base have been added? h) what is the pH of the titration…

Consider the equilibrium shown. SrF, (s) = Sr + (aq) + 2F (aq) K = 2.60 x 10-9 Determine the concentrations of Sr+ and F in a saturated solution of SrF, in pure water (assume u = 0M). !3! [S?*1 = M [F] = Determine the concentrations of Sr+ and F in a saturated solution of SrF, in a solution with an ionic strength of 0.010 M. [Sr*] = [F] = M

The weak monoprotic acid, acetic acid, is titrated with the strong base, potassium hydroxide as follows: HC2H3O2(aq) + K+ OH- (aq) → K+ C2H3O2-(aq) + H2O(l) Ka for acetic acid is 1.81 x 10-5 (at 25 oC). A 25.00 mL sample of a solution of acetic acid with concentration 0.0833 M is titrated with 0.1000 M KOH. A. What is the pH at the beginning of the titration, Vbase = 0.00 mL? B. What is the pH at the equivalence point? C. What is the pH of the titration when 5.00 mL of base have been added? D. What is the pH when the volume of base added equals half the volume of the equivalence point?  E. What is the pH of the titration when 20.00 mL of base have been added? F. What is the pH of the titration when 30.00 mL of base have been added?

A completely made up compound of fluoride, XC12, is found to have a molar solubility of 8.31 x 10-23, when dissolved in an 2.43 M AICI3 (aq) solution. What is the Ken for this compound? Please input your answer to the second decimal place. Type your answer.

estion 6 Solid nickel (II) acetate is slowly added to 125 mL of 0.00846 M ammonium carbonate solution. What is the concentration of nickel (II) ions required to just initiate precipitation? The Ksp of NICO3 is 6.6 10-9 Report your answer in scientific notation to two significant figures (for example: 0.0012 can be entered as 1.2E-3) Do not input a unit! A Moving to another question will save this response. LEGO 10 R] H. B N. 0

PbCl2; molar solubility = 1.43 x 10-² M Ksp = 1.17 Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining Note that Ksp is the solubility-product constant, the equilibrium constant for a chemical equation representing the dissolution of an ionic compound: Ksp = [Pb²+][C1-1² ■√ ΑΣΦ 10-8 Part C Prepare an ICE table (where I means initial, C means change, and E means equilibrium), where the equilibrium concentrations of the formed ions are expressed in terms of S (the number of moles per liter of PbCl2 dissolved) and substitute them into the expression for Ksp. Ksp CaF2; molar solubility = 3.32 × 10-4 M = Submit ΑΣΦ Request Answer

Initial (M) Change (M) Equilibrium (M) Determine the value of Ksp for Aglo, by constructing an ICE table, writing the solubility constant expression, and solving the expression. Complete Parts 1-2 before submitting your answer. 2 NEXT It is found that up to 0.0980 g of AglO, dissolves in 2.00 L of aqueous solution at a certain temperature. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products at this temperature. -0.0490 0 -1.73 x 10* AgIO,(s) Question 2 of 10 0.0980 -3.47 x 10* 0.0490 -1.73 x 10³ 1.73 x 10* Ag (aq) 3.47 x 10* 1.73 x 10- RESET -0.0980 10, (aq)

Determine the solubility of aluminum hydroxide, Al(OH)3, in a buffer solution at a pH of 7.Ksp = 3.7E-15Include at least 3 significant figures in your answer.