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Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of K2S and Fe(NO3)2 are mixed. Fe^2+(aq) + S^2-(aq) rightarrow FeS(s) Fe^2+(aq) + S^2-(aq) + 2 K^+(aq) + 2 NO3^-(aq) rightarrow FeS(s) + 2 K^+(aq) + 2 NO3^-(aq) K^+(aq) + NO3^-(aq) rightarrow KNO3(s) Fe^2+(aq) + S^2-(aq) + 2 K^+(aq) + 2 NO3^-(aq) rightarrow Fe^2+(aq) + S^2-(aq) + 2 KNO3(s) No reaction occurs. When 280. mL of 1.50 Times 10^-4 M hydrochloric acid is added to 135 mL of 1.75 times 10^-4 M Mg(OH)2, the resulting solution will be: neutral. acidic. basic It is impossible to tell from the information given. Which of the following is an oxidation-reduction reaction? Nal(aq) + AgNO3(aq) rightarrow Agl(s) + NaNO3(aq) Mg(s) + 2 HCI(aq) rightarrow MgCl2(aq) + H2(g) Hl(aq) + LiOH(aq) rightarrow Lil(aq) + H2O(l) Pb(C2H3O2)2(aq) + 2 NaCI(aq) rightarrow PbCl2(s) + 2 NaC2H3O2(aq) All of the above are oxidation-reduction reactions. Determine the oxidation state of nitrogen in LiNO3. +5 +3 0 +2 +4 What element is defined by the following information? p^+ = 20 ndegree = 20 e^- = 20 zirconium calcium neon argon potassium

Explanation / Answer

1)

K2S + Fe(NO3)2 --> FeS + 2KNO3

Net ionic are those that acutally react so

S-2 + Fe+2 --> FeS(s)

2)

mmol of acid = M*V = 280*(1.5*10^-4) = 0.042

mmol of base = 2*135*(1.75*10^-4)= =0.04725

since there ar emol of base, expec this to be basic

3)

redox -> chang eon oxidation numbers

a) not redox, jsut double replacement

b) redox, since Mg 0 -> Mg+2

c) acid-base, not redox

d) double replacement, not redox

4)

LiNO3

Li +1

O = -2

then

+1 + N + 3*-2 = 0

N = +5

5)

Z= 20

then

must be calcium

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