1. Calculate the solubility of ZnC204 in a solution held at pH 4.00. Consider the equilibria ZnC204(s) Zn2+ + C2042- C2O4 + H2O HC204 + OH HC2O4 + H2O H2C2O4 + OH¯ Ksp = 7.5 x 10-9 Kb1 = 1.8 x 10-10 Kb2 = 1.8 x 10-13
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- The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSeO4, 0.0118 g/100 mL. (b) Ba(BrO3)2H2O, 0.30 g/100 mL. (c) NH4MgAsO46H2O, 0.033 g/100 mL. (d) La2(MoO4)3, 0.00179 g/100 mLCalculate the molar solubility of SrC2O4 in a solution that has a fixed H3O+ concentration of (Ksp (SrC204) = 5.0 × 108, K₁ (H2C2O4) = 5.60 x 102, K2(H2C2O4) = 5.42 × 10-5) a. 8.0 × 10-6 M. Molar solubility= M b. 8.0 × 107 M. Molar solubility = c. 8.0 x 109 M. Molar solubility = d. 8.0 x 10-11 M. Molar solubility = M M MA chemistry graduate student is given 250. ml. of a 0.80 M diethylamine (C2H5)2NH2Br solution. Diethylamine-3 is a weak base with K, = 1.3 x 10 • What mass of (C2H5)2NH2Br should the student dissolve in the (C2H5)2NH solution to turn it into a buffer with pH = 10.92? You may assume that the volume of the solution doesn't change when the (C2H5)2NH2Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
- ys 111111Determine the molar solubility of AgSCN in a solution maintained at pH 11.00 and where the concentration of free ammonia is 0.100 M. AgSCN: Ksp = 1.1 x 10-12HSCN: pKa = 4.0[Ag(NH3)2]+: Kf1 = 2.04 x 103 ; Kf2 = 8.13 x 103Calculate the molar solubility of AgSCN (Ksp = 1.1 x 10^-12) in a solution maintained at pH 9.00 and where the concentration of ammonia is 0.1 M. HSCN: pKa = 4.0 [Ag(NH3)2]^+ : Kf1 = 2.04 x 10^3; Kf2 = 8.13 x 10^3
- Find the molar solubility of Ag2CO3 when the concentration of [H3O +] is 1.0x10 ^ 11 M. (Ksp for Ag2CO3 = 8.1x10 ^ 12 Ka1 = 4.45x10 ^ 7 Ka2 = 4.69x10 ^ 11 for H2CO3)A buffer was made with HC2H3O2 and its conjugate base. What is the pH of the buffer if at equilibrium there was [HC2H3O2] = 0.5000 M and [C2H302ª] = 0.7000 M and the Ka = 1.60 x 10-5 ? everything is based upon the acid dissolving in water: HC2H3O2 + H20 C2H3O21 + H30*1 [ Ka = [ solve for [H30*'] then put in the numbers Ka [ ( [H3O+1] : [ ] [H3O+'] = pH = - log d. HC6H6O61 f. SO3? a. H30+1 b. Он1 c. H2C6H606 е. HSO31 -2 g. H2SO3 h. HC2H3O2 i. C2H3O21 j. H2S k. HS-1 I. s2 m. HX п. X-1 О. 1 р. 2 q. 3 r. 0.5000 s. 5.5 X 10-5 t. 3.5 X 10-4 u. 8.00 x 10-5 v. 1.75 x 10-6 w. 1.11 x 10-8 х. 5.5 х 102 y. 0.7000 z. 1.60 x 10-5 аа. 1.143 х 10-5 bb. 0.4900 сс. 1.104 х 10-5 dd. 0.7100 ее. 1.26 х 10-5 ff. 4.901 gg. 7.93 hh. 4.942 ii. 4.957A buffer was created using ascorbic acid and sodium ascorbate. What is the pH of the buffered solution if at equilibrium [H₂C6H6O6] = 5.5 X 10-5 M, [HC6HO6¹¹] = 3.5 X 104 M, and K₂ = 8.00 x 10-5 ? everything is based upon the acid dissolving in water: H₂C6H6O6 + H₂O HC6H6O6¹¹ + H3O+1 [ |][ Ka = [ solve for [H3O+¹] then put in the numbers Ka [ [H3O+¹] = [ [H3O+¹] = pH = -log a. H30+1 b. OH-1 h. HCzH3O2 i. C₂H3O₂-¹ = c. H₂C6H6O6 q. 3 r. 0.5000 s. 5.5 X 10-5 x. 5.5 x 10-² dd. 0.7100 ] y. 0.7000 z. 1.60 x 10-5 ee. 1.26 x 10-5 ff. 4.901 ( d. HC6H606¹¹ j. H₂S k. HS-1 t. 3.5 X 10-4 -1 e. HSO3¹¹ 1. S-² X( m. HX f. SO3² n. X-1 g. H₂SO3 o. 1 p. 2 W. 1.11 x 10-8 u. 8.00 x 10-5 v. 1.75 x 10-6 aa. 1.143 x 105 bb. 0.4900 cc. 1.104 x 10-5 gg. 7.93 hh. 4.942 ii. 4.957
- Find the molar solubility of Ag2CO3 since the concentration of [H3O+] is 1.0x10-11 M.(Ksp = 8.1x10-12 for Ag2CO3; Ka1 = 4.45x10-7; Ka2 = 4.69x10-11 for H2CO3)For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K,, data in the ALEKS Data tab. sp compound Does solubility change with pH? highest solubility pH = 9 pH = 8 pH = 6 yes BaCO3 O no ○ yes PbF₂ O ○ no ○ yes CuBr ○ no O X 0 GA 100.0 mL solution containing 0.923 g of maleic acid (MW = 116.072 g/mol) is titrated with 0.306 M KOH. Calculate the pH of the solution after the addition of 52.0 mL of the KOH solution. Maleic acid has pK₂ values of 1.92 and 6.27. pH = At this pH, calculate the concentration of each form of maleic acid in the solution at equilibrium. The three forms of maleic acid are abbreviated as H₂M, HM¯, and M²-, which represent the fully protonated, intermediate, and fully deprotonated forms, respectively. [M²-] = [HM-] = [H₂M] = X- M M M