A chemist wishes to precipitate yttrium cations out of a 1.00 L solution. if the concentration of in solution is 0.428 M and the K of yttrium lodate is 1.12 x 10, what mass of potassium iodate (003 must be added so that precipitation may begin? The molar mass of potassium lodate is 214.00 g/mol. (27) (A) (B) (C) (D) (E) 91.6g 64.0 E (6.4 x 10 g) 411 mg 56.0 ng 137 mg (5.6 x 10 e)

Use the solubility rules to predict whether the following ionic compounds are soluble in water: (a) AgCl; (b) AgNO3; (c) Ca(NO3)2; (d) Ca(OH)2. (a) insoluble (b) soluble (c) soluble (d) soluble 8

18.0 g of zinc is added to 100. mL of 0.200M HBr. a) Will all of the zinc dissolve? b) What will be the concentration of Br in the resulting solution (after any reaction takes place)?

In the following acid-base titration experiment NaOH(aq) + HNO3(aq) ———> NaNO3(aq) + H2O(1). What is the molarity of the HNO3 solution if 18.3 mL of 0.115 M NaOH was used to neutralize 25 mL of HNO3? (a) 0.157 M (b) 0.0842 M (c) 3.978 M (d) 0.0157 M

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Which of the following solutions will produce a precipitate when added to Na2SO4 solution? (A) Ba(NO3)2(aq) (B) Cu(NO3)2(aq) (C) Zn(NO3)2(aq) (D) All the above

Given the following information: acetylsalicylic acid (aspirin) hydrocyanic acid (2) At equilibrium the HC₂H704 HCN Submit Answer (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.536 M aqueous acetylsalicylic acid (aspirin) and sodium cyanide are mixed. It is not necessary to include states such as (aq) or (s). (3) The pH of the resulting solution will be will be favored. = Try Another Version Ka = 3.0x10-4 Ka = 4.0x10 10 seven. + 2 item attempts remaining

A chemist combines 53.9 mL of 0.372 M potassium bromide with 23.1 mL of 0.451 M silver nitrate. (a) How many grams of silver bromide will precipitate? (b) What is the final molarity of the K* ion? (c) What is the final molarity of the silver or bromide ion, whichever one is in excess? (а) g AgBr (b) M K* (c) Мехсess ion

What mass of Fe(OH)3 will be obtained when 100. mL of 0.240 M FeClz is mixed with 200. mL of 0.182 MNAOH? |g Fe(OH)3

You mix aqueous solutions of 100.0 mL 1.70 M NaCl and 75.o mL 1.20 M Pb(NO3)2, calculate the mass of of precipitate formed.