General Chemistry
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Calculate the molar solubility of lead chloride in 0.25 M Pb(NO3)2.
Chloric acid (HClO3) will ionize less than in which solution than it does in pure water?
In which of these solutions will HNO2 ionize less than it does in pure water?
When KOH(aq) is added to the solution, will the solubility of Ni(OH)2 increase, decrease, or remain the same? Give the balanced net ionic equation for the dissolution process. [Hint: Refer to complex ions formations]
Determine whether the pH will change or not in the following scenarios. If the pH changes, identify whether it will increase or decrease.
A. NaBr is added to an HBr solution
B. C6H5NH3Cl is added to a C6H5NH2 solution
C. NaCN is added to an HCN solution
Calculate the molar solubility of PbBr2 (Ksp = 6.6×10–6) in 0.150 M aqueous KBr solution.
Ni(OH)2 is a sparingly soluble hydroxide. Will its solubility increase, decrease, or remain unchanged when a small amount of HBr is added to a solution of Ni(OH)2?
Write a balanced net ionic equation for the dissolution reaction (if it takes place).
What are the molar solubilities of CuC2O4 (Ksp = 4.43×10–10 M) in pure water and in a 2.5×10–3 M Na2C2O4 solution?
Based on Le Chatelier's principle, what will happen to the solubility of AgCN when AgClO4 is added to the solution?
Based on Le Chatelier's principle, what will happen to the solubility of AgCN when KCl is added to the solution?
Based on Le Chatelier's principle, what will happen to the solubility of AgCN when NaCN is added to the solution?
Based on Le Chatelier's principle, what will happen to the solubility of AgCN when HClO4 is added to the solution?
The [Pb2+] and [AsO43−] in a certain saturated Pb3(AsO4)2 solution are both equal to 8.3×10−8. In a saturated solution with [Pb2+] = 0.020 M, what is [AsO43−]?
Consider the following equilibrium reaction
NH3(aq) + H2O(l) ⇌ NH4+(aq) + OH–(aq).
What would happen to the pH of the solution if a salt of NH4+(aq) is added to a solution of NH3(aq) at equilibrium?
The Ksp values for MnCO3 and CuCO3 are 5.0×10–10 and 2.3×10–10, respectively. In a solution that is at equilibrium with both compounds, calculate [CO32–], [Mn2+], and [Cu2+].
Assuming that solid Ag2SO4 (Ksp = 1.2×10–5) is in equilibrium with a Na2SO4 solution, what amount of Na2SO4 in molarity is needed to make a 3.5×10–3 M Ag+ solution?
What is the solubility (in g/L) of Ni(OH)2 (Ksp = 6.0×10–16) in a solution buffered at pH = 5.85?
A beaker contains undissolved MgCl2(s) that is in equilibrium with the saturated solution of MgCl2. If some solid MgBr2 is added to the solution, what would happen to the amount of the solid MgCl2?
AX and AY2 are two slightly soluble salts of A2+. Both of the salts have the same solubility of 6.2×10–5 mol/L. When a saturated solution of AX is added to a saturated solution of AY2, what is the final equilibrium concentration of A2+ in the solution?
Choose the most correct statement about the common-ion effect.
Consider the graphs shown below which show how Mg(OH)2 behaves under different conditions. The y-axis in each graph represents the solubility of Mg(OH)2 and the x-axis represents the concentration of another reagent. Identify the graph that corresponds to the solubility of Mg(OH)2 as HCl is added to the solution.
Cobalt (II) hydroxide is dissolved in a solution buffered at pH = 9.5, calculate the solubility Co(OH)2 (in grams per 1.00×102 mL of solution). Compare this to the solubility of Co(OH)2 in pure water.
If magnesium hydroxide is dissolved in a buffered solution with pH of 5.6, calculate the molar solubility of magnesium hydroxide in the solution.
What is the molar solubility of the ionic compound A2X in 0.15 M Na2X solution? (Ksp A2X = 2.62×10–18)
Silver(I) thiocyanate, AgSCN, is a sparingly soluble salt with a Ksp value of 1.00×10–12.
A. Calculate the solubility of AgSCN, in mol/L units, in pure water.
B. Calculate the solubility of AgSCN, in mol/L units, in 0.150 M KSCN solution.
Calculate the molar solubility of calcium hydroxide in a solution buffered at each pH.
a. pH = 4