Test your skills on the following problems.
Practice: How many milligrams of NaCN are required to prepare 712 mL of 0.250 M NaCN?
Practice: What volume (in μL) of 0.100 M HBr contains 0.170 moles of HBr?
Practice: How many moles of Ca2+ ions are in 0.100 L of a 0.450 M solution of Ca3(PO4)2?
Practice: How many chloride ions are present in 65.5 mL of 0.210 M AlCl3 solution?
Practice: To what final volume would 100 mL of 5.0 M KCl have to be diluted in order to make a solution that is 0.54 M KCl?
Practice: If 880 mL of water is added to 125.0 mL of a 0.770 M HBrO4 solution what is the resulting molarity?
Practice: Consider the following balanced redox equation:
H2O + 2 MnO4 – + 3 SO32– ----> 2 MnO2 + 3 SO42– + 2 OH –
How many grams of MnO2 (MW: 86.94 g/mol) are produced when 32.0 mL of 0.615 M MnO4– (MW: 118.90 g/mol) reacts with excess water and sulfite?
Practice: Iron (III) can be oxidized by an acidic K2Cr2O7 solution according to the net ionic equation:
Cr2O72– + 6 Fe2+ + 14 H+ -----> 2 Cr3+ + 6 Fe3+ + 7 H2O
If it takes 35.0 mL of 0.250 M FeCl2 to titrate 50 mL of a solution containing Cr2O72–, what is the molar concentration of Cr2O72–?
Practice: Vinegar is a solution of acetic acid, CH3COOH, dissolved in water. A 5.54 g sample of vinegar was neutralized by 30.10 mL of 0.100 M NaOH. What is the percent by weight of acetic acid in the vinegar?
Practice: What is the molar mass of a 0.350 g sample of a monoprotic acid if it requires 50.0 mL of 0.440 M Ca(OH)2 to completely neutralize it?
Example #1: Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of sodium sulfide and copper (II) nitrate are mixed.
Example #2: Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of H2SO4 and KOH are mixed.
Example #3: Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Na2CO3 and HCl are mixed.