What mass of AgI dissolves

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%)

If KI was not available to precipitate AgI from AgNO3 then what reagent can be used instead? HNO3 AgNO3 NH3 HI

If 100.0 g calcium phosphate (Ksp= 1.3 x 10^-32) are placed in enough water to generate 750.0 mL of solution, calculate the molar solubility of the calcium phosphate solution and the molar solubility of the calcium ion if 30.0 mL of 0.400 M calcium nitrate solution is added to the original solution.

*76. Using data from Table 16.3, calculate the concentrations of Hg²*(aq), HgCl*(aq), and HgCl2(aq) that result when 1.00 L of a 0.100 M Hg(NO3)2 solution is mixed with an equal volume of a 0.100 M HgCl, solution. (Hint: Use the analogy with amphoteric equilibria discussed in Sec- tion 10.8.)

[CD]d Q = AB K = CD]a Please calculate the molar solubility of Al(OH)3 when dissolved in a pH =3.59 solution, if the K sp for Al(OH)3 is K sp = 2 × 10¬32 Please input your answer in scientific notation to the second decimal place. (If you get back a whole number, like 5.67 just type in 5.67 *10^0) Type your answer...

7. How many grams of ScF3(s) can be dissolved in 100.0 mL of H2O?

Select the compound(s) below that would impact on the solubility of AgBr (silver bromide, a salt):

Magnesium hydroxide is poorly soluble in pure water but dissolves quite well in pH 7.0 buffer. This may be explained by: a) buffers always increase solubility   b) hydroxide ion is being removed from the solution   c)   magnesium ion is being added to the solution   d)  air oxidation of the magnesium ion

17. In which of the following solutions, Mn(OH)2 has the greatest solubility? (by assuming sufficient Mn(OH)2 (s) present in solution). Ksp (Mn(OH)2) 2.0 × 10-13. a) 0.20 M HNO3 b) 0.20 M NaNO3 c) b) 0.20 M Mn(NO3)2 e) same solubility for all