Identify each of these reactions as a precipitation, neutralization or metal displacement: a. ) Zn (s) + CuCl2 (aq) = Cu (s) + ZnCl2 (aq) b.) NaOH (aq) + HBr (aq) = H2O (l) + NaBr (aq) c.) 2 KBr (aq)+ Pb(NO3)2 (aq) = PbBr2 (s) + 2 KNO3 (aq) d.) Ni(NO3)2 (aq) + Ca (s) = Ca(NO3)2 (aq) + Ni (s)

esc What mass of precipitate (in g) is formed when 250.0 mL of 0.300 M MnCl₂ is mixed with excess KOH in the following chemical reaction? MnCl₂(aq) + 2 KOH(aq) → Mn(OH)₂(s) + 2 KCl(aq) Q 25 F1 @ 2 F2 W # #c 20 3 F3 E 000 000 $ 4 ZATO F4 R % 5 F5 T tv A MacBook Air ^ 6 F6 & 7 F7 8 11 W F8 1

A 25.00 mL Ba(OH), solution of unknown concentration was neutralized by the addition of 29.27 mL of a 0.1460 M HCI Psolution. Write the balanced molecular equation for the neutralization reaction between HCI and Ba(OH)2 physical states. in aqueous solution. Include molecular equation: Ba(OH)2(aq) + 2HCl(aq) → BaCl2(aq) + 2H2O(1) Calculate the concentration of Ba(OH)2 in the original 25.00 mL solution. [Ba(OH)2] = 0.085 Calculate the concentrations of Ba2+ and Cl in solution following the neutralization reaction. [Ba²+] = [CI] = M M M

A 38.5 mL sample of 0.875M AgNO3 solution is mixed with 51.0mL sample of 0.744M NaCl solution. The AgCl precipitated has a mass of 2.06g. Calculate the limiting reactant, the theoretical yield, and the percent yield.AgNO3 (aq) + NaCl (aq) ---> AgCl (s) + NaNO3 (aq)