1. For each of the following, explain whether the substances can form a solution
ID: 559629 • Letter: 1
Question
1. For each of the following, explain whether the substances can form a solution or not.
A. NH3 and NaCl CH4
B. KBr C4H10
C. CO2
2. Classify the following compounds as strong electrolytes, weak electrolytes or non-electrolytes based on their dissolution reactions in water.
A. C6H12O6(s)C6H12O6(aq)
B. Na3PO4(s)3 Na(aq)+PO43(aq)
C. AgCl(s)Ag+(aq)+Cl+(aq)
D. Mg(NO3)2(s)Mg2+(aq)+2 NO3-(aq)
3. Write the balanced total ionic equation and net ionic equation for the reaction that occurs when and (NH4)2CO3(aq) and MgSO4(aq) are mixed.
4. What is the molarity of a solution in which you dissolve 45.9 g CuSO4(s) in 3.25 L of water?
5. What is the molarity of an acetic acid (C2H4O2) solution in which 95.0 g of acetic acid is dissolved in 150.00 mL of water?
6. Given 300. g of a 27.5% m/m solution of NaCl(aq), how many moles of NaCl do you have?
7. You react 9.00 mL of 0.750 M Hg2(ClO3)2(aq) with an unlimited supply of a 0.100 M solution of NaCl which will produce Hg2Cl2(s) and NaClO3(aq).
A. Write the balanced chemical equation.
B. How many grams of Hg2Cl2(s) could you theoretically produce?
C. Assuming your reaction has a yield of 87.0%, how many liters of 0.100 M NaCl(aq) would you need to add to remove the mercury(I)?
8. You dilute a 15.0 mL of a 12.0 M solution of BaCl2(aq) by adding 75.0 mL of water. What is the molarity of the diluted solution?
9. Calculate the freezing point of a solution containing 48.5 g CaCl2 in 1.00 kg of water. Note, water’s freezing point decreases by 1.86 °C for every 1 mole of particles dissolved in it.
Explanation / Answer
1. For each of the following, explain whether the substances can form a solution or not.
A. NH3 and NaCl CH4 --> only NH3 and NaCl will; CH4 is gas, will not be soluble in polar compounds
B. KBr C4H10 --> not likely ionic + nonpolar will not form solutions
C. CO2 --> not likely CO2 is not that soluble in water
2. Classify the following compounds as strong electrolytes, weak electrolytes or non-electrolytes based on their dissolution reactions in water.
A. C6H12O6(s)C6H12O6(aq) not eletrolyte, will not form 100% ions
B. Na3PO4(s)3 Na(aq)+PO43(aq) --> strong electroltye, 100% ions
C. AgCl(s)Ag+(aq)+Cl+(aq) --> weak electrolyte, since this is not likely to occur ( euqilibrium shifted)
D. Mg(NO3)2(s)Mg2+(aq)+2 NO3-(aq) --> 100% ionizaiton, implies very strong electrolyte.
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.