Use the solubility table to answer the following. You do not need to mix any che

Question

Use the solubility table to answer the following. You do not need to mix any chemicals. Circle the following solutions that will form a prepriate with addition of HCl(aq) Circle all of the following solutions that will form a precipitate with addition of Mg(IO_3)z(aq) Circle all of the following solutions that will form a precipitate with addition of Ag_2 SO_4(aq) Write the precipitate(s) that will form and remain when the following solutions are mixed: A student divides an unknown compound into three test tubes and performs these tests: When Na_2CO_3 is added to the first tube there is a precipitate When excess Pb(NO_3) is added to the second tube there is a precipitate When excess H_2SO_4 is added to the third tube there is a precipitate The compound could be

Explanation / Answer

1.

AgNO3 (aq )+ HCl (aq) --- > AgCl (S)+ HNO3 (aq)

Ag(aq )+ NO3- (aq )+ H+(aq )+ Cl- (aq) --- > AgCl (S)+ H+(aq )+ NO3- (aq)

Ag(aq)+ Cl- (aq) --- > AgCl (S)

Pb(NO3)2(aq) + 2HCl(aq) PbCl2(s) + 2HNO3(aq)

Pb2+(aq )+ 2NO3- (aq )+ 2H+(aq )+2 Cl- (aq) --- > PbCl2 (S)+2 H+(aq )+ NO3- (aq)

Pb2+(aq)+2 Cl- (aq) --- > PbCl2 (S)

Thus AgNO3 and Pb(NO3)2 gives precipitate with addition of HCl.

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