Calculating the solubility of an ionic compound when a commo. BaCrO 1.17x10-10 Calculate the solubility at 25 "C of AgCI in pure water and in a 0.0030M AGNO, solution. Baso4 1.08 10-10 Caco, 3.36x10- Round both of your answers to 2 significant digits. Cafa 3.45x10-11 5.92x10-15 Co(OH)2 solubility in pure water: Cur 6.27x10- Cuco 14x10-10 solubility in 0.0030 M AgNO, solution: 0: Fe(OH)a 4.8710-17 PECO 740x10-14 2.8x10-13 3.310- 5.61 10-12 NCOH)a 5.4810-16 Agbros 5.3810-5 AgCO 84610-12 Ag 1.7710-10 AgCro 1.1210-12 Srcoy 5.60 10-10

AgCl has a Ksp= 1.8×10−10. If the [Ag+] = 1.0 x 10−5M and [Cl−] = 1.9x 10−5M in a solution will a precipitate of AgCl form? Show all work which justifiesyour answer.

Calculate the mass of precipitate formed after 54 mL of 0.68M Na3PO4 is mixed with 34 mL of 0.84M CaBr₂ ab Edit Format Table 12pt Paragraph esc s lock A control ! 1 Q A 1 option BIUA 2 N W S #3 X E command D ✓ T² v $ 4 R C % 5 F ܀ I T V 8 MacBook Pro < 6 G Y B & 7 H U * : 0 0 words 8 N J ( 1 a 9 K M ) 0 O MOSISO

When 200.0 mL of 5.15 x 10-4 M Ba(NO3)2 is added to 150.0 mL of 8.25 x 10-4 M Na2SO4. Ksp(BaSO4) = 1.08 x 10-10. A precipitate choose your answer.... Ksp because Qsp choose your answer... choose your answer... SIGMA = form

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A fictional compound AX2 has a molar mass of 152.01 g/mol and a Ksp of 5.6237e-10. It dissociates in water based on the equation:AX2(s) ⇔ A2+(aq) + 2X-(aq)Based on this information, label the statements below as true or false.    The mass solubility of AX2 is less than 1.52E-2 g/100mL H2O.    If the solution is heated and the solubility increases, then the heat of solution for AX2 is exothermic.    If soluble NaX is added to the system then [A2+] will increase.    The molar solubility of AX2 is greater than 2.40E-4 mol/L.    If more soluble A(NO3)2 is added to the system then [X-] will decrease.    If more solid AX2 is added to the system then [X-] will increase.    If more solid AX2 is added to the system then [A2+] will increase.

A solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10M in AgNO3 and 0.075M in NaCl. What will happen once these solutions are mixed? Ksp(AgCl)=1.77•10-10.  A) nothing will happen since the molar solubility of AgCl is higher than the solution concentrations. B) silver chloride will precipitate out of solution, leaving an unsaturated solution of AgCl. C) silver chloride will precipitate out of solution, leaving a saturated AgCl solution. D) nothing will happen since NaCl and AgNO3 are both soluble compounds. E) there's not enough information to say anything.

For Ag2S, the solubility product constant, Kgp, is 6×10°30. What is the molar solubility of Ag2S? 2x10-^-15 M 2x10^-30 M 1x10^-10 M 2x10A-10 M

Question 19 of 25 The molar solubility of Mg(CN)2 is 1.4 x 10-5 M at a certain temperature. Determine the value of Ksp for Mg(CN). NEXT Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. Mg(CN) (s) Mg (aq) 2 CN-(aq) Initial (M) Change (M) Equilibrium (M) O RESET 1.4 x 105 -1.4 x 10-5 2.8 x 10-5 -2.8 x 10-5 +x +2x -2x 1.4 x 10-5 + x 1.4 x 10- + 2x 1.4 x 10-5 - x 1.4 x 10 - 2x 2.8 x 10-5 + x 2.8 x 10+ 2r -x 2.8 x 10-5 - x 2.8 x 10 - 2x

5, Calculate the molar solubility of Cobalt(II) hydroxide (blue) Co(OH)2 in pure water                              [ Select ]                          ["4.11x10-4", "1.14x10-5", "2.54x10-6", "5.24x10-3"]            in 0.50M NaOH                              [ Select ]                          ["2.37x10-10", "7.32x10-13", "2.37x10-14", "3.27x10-7"]            Ksp of Co(OH)2 = 5.92 ⋅ 10–15   6, In the supersaturated solution Group of answer choices Q = Ksp Q < Ksp Q > Ksp Ka = Ksp Calculate the pH of a buffer solution prepared by mixing 25 mL 0.400 M butyric acid, HC4H7O2 and 35 mL of 0.200 M potassium butyrate, KC4H7O2. Ka of butyric acid is 2.76 x 10-6. Group of answer choices 5.40 3.60 6.30 4.50