Question

Part A

To what volume should you dilute 20 mL of a 12.0 M H2SO4 solution to obtain a 0.130 M H2SO4 solution?

Express your answer using two significant figures.

Part A

Classify the following reactions:

HCl(aq)+NaOH(aq)→NaCl(aq)+H2O(l)

Ba(OH)2(aq)+ZnCl2(aq)→BaCl2(aq)+Zn(OH)2(s)

2AgNO3(aq)+Mg(s)→Mg(NO3)2(aq)+2Ag(s)

Drag the appropriate items to their respective bins.

Answer 1

part A
use dilution law

M1V1 = M2V2
intital volume = 20 ml
initial molarity = 12 M

final volume V2 =?
final molarity M2 = 0.13 M

V2 = M1V1/V2 = 20 ml* 12M/0.130 M = 1846.ml

round to 2 sig fig

volume = 1800 ml
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HCl(aq)+NaOH(aq)→NaCl(aq)+H2O(l) : Salt and water formed from acid
and base reaction : So It is acid base reaction

Ba(OH)2(aq)+ZnCl2(aq)→BaCl2(aq)+Zn(OH)2(s) : Precipitate formed
Hence it is precipitation reaction

2AgNO3(aq)+Mg(s)→Mg(NO3)2(aq)+2Ag(s) : Mg displaced Ag+ from the salt
So it is single displacement reaction . It is a redox reaction
also

answered by: anonymous