J. Muench WORKSHEET #5 ______________________ CHEM 161 name 1. Decide whether each of the following is a strong acid, weak acid, strong base, weak base, or neutral. Then decide whether it would be classified as a strong electrolyte, weak electrolyte, or non-electrolyte. Substance Acid / Base / Neutral Electrolyte KBr HCHO2 LiOH CH3OH HNO3 NH3 2. Based on the activity series, predict the outcome of the possible single replacement reactions. Then write a net ionic equation for the reaction. If no reaction, write N.R. (there is one). a. Sn(s) + AgNO3(aq) b. Cu(s) + NiCl2(aq) c. Zn(s) + HCl(aq) 3. Using the solubility rules, decide whether the following are soluble or insoluble. a. AgNO3 b. Ni(OH)2 c. CaS d. PbSO4J. Muench 4. Write complete balanced molecular reactions and net ionic reactions for the possible reactions below. If all products are aqueous (soluble), then write N.R. for no reaction (there is one of these). Show your work on the space provided or attach if necessary. a. Cr(NO3)3(aq) + Na2S(aq) b. HBr(aq) + NaHCO3(aq) c. SrBr2(aq) + Na3PO4(aq) d. CuSO4(aq) + NaOH(aq) e. BaCO3(s) + HCl(aq) f. NaNO3(aq) + Li2SO4(aq) 5. Determine what is oxidized and what is reduced in the following reactions. a. 2Al(s) + 3Br2(l) 2AlBr3(s) b. Ni(s) + CdCl2(aq) NiCl2(aq) + Cd(s) c. Fe2O3(s) + 3 CO(g) 2 Fe(s) + 3 CO2(g)J. Muench 6. A 20.0mL sample containing the weak acid HC7H5O2 is titrated to determine the amount of acid present. If the acid solution required 28.3mL of a 0.126M NaOH solution to reach the endpoint, then: HC7H5O2(aq) + NaOH(aq) H2O(l) + NaC7H5O2(aq) a. determine the concentration of the acid solution. b. determine the mass of acid present in the solution. 7. A 50.0mL sample of Ca(OH)2 solution requires 145.2mL of a 0.0525M HCl solution to reach the endpoint. What mass of Ca(OH)2 is present in the solution? The reaction is: Ca(OH)2(s) + 2 HCl(aq) 2 H2O(l) + CaCl2(aq) 8. A 3.33g sample of iron ore is treated with concentrated H2SO4, which converts the iron to FeSO4. If this solution is then titrated with 41.4mL of a 0.150 M K2Cr2O7 solution, then what is the percentage of iron present in the sample? The balanced reaction is: 6FeSO4(aq) + K2Cr2O7(aq) + 7H2SO4(aq) 3Fe2(SO4)3(aq) + Cr2(SO4)3(aq) + 7H2O(l) +