(a) Iz(s) + 5 Cu²* (aq) + 6 H2O(1) (b) Hg²*(aq) + 21 (aq) (c) H2SO3(aq) + 2 Mn(s) + 4 H*(aq) → S(s) + 2 Mn²* (aq) + 3 H,O(I) 2 10;"(aq) + 5 Cu(s) + 12 H*(aq) - Hg(1) + I2(s) - -

A chemist performs a gravimetric analysis. The chemist combines 1.00 L of 2.00 M AGNO, (ag) with 1.00 L of 4.00M NaCl (ag) in an Erlenmeyer flask. Both the AgNO3 (aq) solution and the NaCl(aq) solution are colorless. After the mixture has been stirred, a cloudy white substance is observed at the bottom of the flask. What is the expected mass of AgCl (s), in grams, assuming that the yield is 100%? In the box, enter the mass to the nearest gram.

In the following chemical reaction, which element is the reducing agent? 2 Ag(s) + 2CI(aq) + 2 H,O(1) → 2 AGCI(s) + H,(g) + 2 OH (aq) A) Ag B) CI C) H D) O

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

In the reaction AgNO3(aq) + KI(aq) → AgI(s) + KNO3(aq) which ions are the spectator ions?

Please don't provide handwritten solution

2+ (a) MnO + VO²+ → Mn²+ + V(OH)4+ (b) I₂ + H₂S(g) → I¯¯ +S(s) 2+ (c) Cr₂O7²- + U4+ → Cr³+ + UO₂²+ (d) Cl + MnO₂ (s) → Cl₂(g) + Mn²+ (e) IO3 + I→ 1₂(aq) (f) IO3 + I + Cl¯ → IC₂ (g) HPO3²- + MnO4+OH → PO³+ MnO2- Write balanced redox equations for the following reactions. Show the full balancing process and supply H+ and/or H2O as needed to obtain balance. Item g is balanced in basic medium while the rest are in acidic medium. Identify the oxidizing agent and the reducing agent on the left side of each equation in the previous problem.

To measure the concentration of an aqueous solution ofH2O2, an analytical chemist adds strong acid to a 39.00g sample of the solution and titrates it to the endpoint with 49.5mL of 0.2700M potassium permanganate KMnO4 solution. The balanced chemical equation for the reaction is: 6H+(aq) + 5H2O2(aq) + 2MnO−4(aq) -> 5O2(g) + 2Mn2+(aq)  8H2O(l)   What kind of reaction is this?  If you said this was a precipitation reaction, enter the chemical formula of the precipitate. If you said this was an acid-base reaction, enter the chemical formula of the reactant that is acting as the base. If you said this was a redox reaction, enter the chemical symbol of the element that is oxidized.   Calculate the mass percent of H2O2 in the sample. Be sure your answer has the correct number of significant digits.

The amount of I, (aq) in a solution can be determined by titration with a solution containing a known concentration of S,0 (aq) (thiosulfate ion). The determination is based on the net ionic equation 2 S,03 (aq) + I5(aq) → S,0 (aq) + 31(aq) Given that it requires 30.1 mL of 0.310 M Na, S,O, (aq) to titrate a 15.0 mL sample of I, (aq), calculate the molarity of I, (aq) in the solution. [I]= Question Source: MRG - General Chemistry Publisher: University Science Books

The concentration of Sn²+ in a solution is determined by titrating it with a 0.1890 M permanganate solution. The balanced net ionic equation for the reaction is: 2MnOq°(aq) + 5Sn²*(aq) + 16H3O*(aq) → 2Mn²+(aq) + 5Sn*(aq) + 24H,O(1) In one experiment, 24.99 mL of the 0.1890-M permanganate solution is required to react completely with 40.00 mL of the Sn2+ solution. Calculate the concentration of the Sn2+ solution. M