sample of cadmium weighing 3.139 g is dissolved in 3.00 M HCl. What (minimum) volume of HCl is required to dissolve the Cd? (Cd dissolves in HCl to form Cd2+)

Calculate the concentration (molarity) of Pb2+ ions in a solution made by adding 0.010 moles of Pb(NO3)2 to 1.0 L of a  2.0 M NaI solution.  (Kf = 3.0 x 104 for PbI42−) - 4.9 x 10−2 -3.3 x 10−5 - 2.1 x 10−7 -1.7 x 10−7 -2.3 x 10−8

A solution is titrated with AgNO, to determine the CI concentration. At the endpoint is a colloidal suspension of AgCl in a slight excess of Ag* and NO, ions. Which of the procedures would promote coagulation of the particles so that the precipitate can be filtered and weighed? heating the suspension adding more AGNO, solution cooling the suspension adding an electrolyte such as 0.1 mol HNO, adding more NaCl solution

A solution contains 1.0 x 10−5 M Na3PO4. What is the minimum concentration of AgNO3 that would cause precipitation of solid Ag3PO4? (Ksp = 1.8 x 10−18)

A  solution is made by dissolving 0.053g of Ag CL into 1.00 kg of solvent. What is the concentration of the solution in PPM??

2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)

In which of the following solutions would PbBr₂ be the most soluble? O 0.10 M Pb(NO3)2 O 0.20 M KNO3 0 0.15 M NaBr

3. A buffer system containing H2PO4– and HPO42– helps regulate the pH of cytoplasm in living cells. What is the mole ratio of HPO42– ions to H2PO4– ions in a buffer with a pH of 7.80? Ka of H2PO4– is 6.5 × 10–8