Determine the molar solubility for Al(OH)3. Write a balanced dissociation equation for Al(OH)3 in aqeuous solution. If the compound does not dissociate, write NR after the reaction arrow. Be sure to include the proper phases for all species within the reaction. 1 +: 2 0₂ 3 NR Question 9.a of 16 4 5 6 7 口。 0₂ 7 OOOOO = OH (1) 3+ 4+ 8 8 9 0 9 Do (g) (aq) Al

Determine the compound that is expected to be more soluble in acidic solution than in neutral or basic solution. О KBr O BaCl2 O Ni(OH)2 O Cu(NO3)2

What is the ratio of the moles of sodium hydroxide to the moles of crystal violet (nNaOH/nCV+) at the start of the reaction? Make sure to account for the fact that different volumes of the stock solutions are mixed. 5.0 mL 2.0 × 10–5 M crystal violet solution 1.0 mL of 0.10 M NaOH solution Trail. [Na+]j (M) [OH–]j (M) 1 1.67 × 10–2 1.67 × 10–2

Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. NEXT > The buffer was prepared by dissolving 21.5 g HC,H,O₂ and 37.7 g of NaC,H,O₂ in 200.0 mL of solution. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) 0.178 0.880-x [0] [0.888] [1.31 + x) 0 0 0.888 1.31 + x HC₂H5O₂(aq) + [21.5] [x] Ka = 4.2 x 10-² 21.5 0.178 + x +x [37.7] [2x] 1 [0.178+x][0.888 + x] 37.7 -x 0.888 + x Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. 6.23 The Ka for HC₂H5O₂ is 6.3 x 10-5. Based on your ICE table (Part 1) and the definition of Ka, set up the expression for Ka…

1. How do you prepare a 100mL of 0.1 M phosphate buffer?To make 100 mL of 0.1 M phosphate buffer: Calculate the amount of sodium phosphate needed. moles of sodium phosphate = (0.1 mol/L) x (0.1 L) = 0.01 moles mass of sodium phosphate = moles x molar mass = 0.01 moles x 142 g/mol = 1.42 g Dissolve 1.42 g of sodium phosphate in distilled water in a 100 mL volumetric flask. Adjust the pH of the solution to the desired value (usually around 7.4) using a strong acid or strong base. Bring the solution to the final volume (100 mL) with distilled water.   2. From the anterior buffer, how do you make 100mL of 0.05 M? To make 100 mL of 0.05 M phosphate buffer from the 0.1 M stock solution: Calculate the amount of the 0.1 M phosphate buffer needed. moles of phosphate buffer = (0.05 mol/L) x (0.1 L) = 0.005 moles Calculate the volume of the 0.1 M phosphate buffer needed. moles = concentration x volume (in liters) volume = moles / concentration = 0.005 moles / 0.1 mol/L = 0.05 L or 50 mL Measure…

A solution is prepared that is initially 0.27M in acetic acid (HCH3CO2) and 0.053M in potassium acetate (KCH3CO2). Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in [H₂O]. You can leave out the M symbol for molarity. [HCH2CO₂] cu_co, [H₂O*] initial change final

The silver-ion concentration in a saturated solution of silver(1) sulfate is 2.9 x 10-2 M. What is Ksp for silver(1) sulfate? 2.1 x 104 8.3 x 10-4 1.2 x 10-5 9.8 x 10-5 6.9 x 10-7

The solubility product for silver (I) bromide is 7.7 × 10–13.  Calculate the molar solubility of silver (I) bromide.

5) Calculate the solubility of each of the following salts in moles per liter given their Ksp values. Ignore any acid-base properties.a. Ag3PO4, Ksp=1.8x10−18b. CaCO3, Ksp=8.7x10−9C) Calculate the solubility of the silver phosphate and the calcium carbonate in question 5 in grams/L.

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