A student added 1 mL of 0.01 M KMnO4 with 6 drops of 6 M NaOH and then added drops of fresh aqueous 0.1 M FeSO4. The student observed the formation of a muddy black precipitate. Based on the experimental observation, determine the balanced net ionic equation for the reaction that occurred.

If 0.750 L of a 0.0010 M of AgNO3 is added to 0.500 litre of a 0.00050 M solution of CaF2, what is the concentration of each ion after mixing? A solution of Ca (NO) is added to a solution of NazCO. Write down the balanced 3 reactions showing what happens in solution. What is the precipitate? A solution of Pb(CH COO) is added to a dilute solution of MgSO4. Write down the balanced 3 reactions showing what happens in solution. What is the precipitate?

A solution contains 7.52x10 M sodiumn bromide and 9.10×103 M ammonium cyanide. Solid silver acetate is added slowly to this mixture. What is the concentration of cyanide ion when bromide ion begins to precipitate? [cyanide] = Submit Answer Retry Entire Group 8 more group attempts remaining

Use solubility to calculate Ksp. The solubility of Co(OH)₂ is measured and found to be 3.75×104 g/L. Use this information to calculate a Ksp value for cobalt(II) hydroxide. Ksp =

Complete the following solubility constant expression for PbCrO 4. K sp = 0 X Ś

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Determine the number of grams of PbCl2 produced from 100.0 ml of 0.20 M Pb(NO3)2 and sufficient NaCl in the following precipitate reaction  2 NaCl + Pb(NO3)2 --> PbCl2 + 2 Na(NO3)

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%)

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The solubility product constant for CaCO3 (s) in water is Ksp = [Ca+2] [CO3 -2] = 4.8 x 10^-9 Consider a 1.00 M solution of calcium chloride, in which you drop a piece of Dry Ice. Show that the minimum concentration (threshold amount) of carbonate ions necessary for a precipitate to appear is 4.8 x 10-9 M. Another way to think about this situation is to calculate the Q for the calcium chloride/Dry Ice solution and ask “will precipitation occur?”..