Calculate the molarity of a sol prepared by dissolving 110.0 mg of KMhO4(158 g/mol) in enough water to make 150.0 solution. The solution will be used to oxidize FeCl2 according to the following reaction (unbalanced): KMNO4 + FeCl2+ HCI → MnO2+ FeCl3 + H20 + KCI O 4.64 x 10-3M O 2.32x 10-2 M 4.46 x 10-3 M

Please write the whole reducing and oxidizing agents. This will help me

One way to determine the hardness of a water sample is to precipitate the calcium out of solution as a carbonate.  The net ionic reaction for this precipitation is:                         Ca2+(aq)  +  CO32-(aq)  →  CaCO3 (s)   A 1.00 L sample of water is drawn from a Phoenix, AZ well and 0.534 g of calcium carbonate is recovered using the above reaction. What was the Ca2+ concentration of the original water sample in ppm? Show your work and include units.  Hint:  ppm stands for parts per million, and in the case of an aqueous solution, this is equivalent to mg/L.

For the reaction:     Fe +      H2SO4 ⟹⟹      Fe2(SO4)3 +      H2   1. Identify the type of reaction as acid-base, oxidation-reduction, or precipitation 2. Balance the chemical equation

Consider the following balanced redox reaction:              16H+(aq) + 2MnO4-(aq) + 10Cl-(aq) →                                                                  2Mn2+(aq) + 5Cl2(g) + 8H2O(l) What species is the reducing agent? What species is the oxidizing agent?

Decide whether each chemical reaction in the table below is an oxidation-reduction ("redox") reaction. If the reaction is a redox reaction, write down the formula of the reducing agent and the formula of the oxidizing agent.

For the oxidation-reduction reaction equation 4 Ga + P → 4 GaP 4 indicate how many electrons are transferred in the formation of one formula unit of product. electrons:

4

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of H 2C 2O 4 and H 2O in the balanced reaction? MnO 4⁻( aq) + H 2C 2O 4( aq) → Mn 2+( aq) + CO 2( g)     H2C2O4 = 5, H2O = 8     H2C2O4 = 1, H2O = 4     H2C2O4 = 5, H2O = 1     H2C2O4 = 1, H2O = 1     H2C2O4 = 3, H2O = 2

Complete and balance the following redox equations using the smallest whole-number coefficients. The reaction takes place in a BASIC solution. Fe(OH)2 (s) + MnO4−(aq)  →  MnO2 (s) + Fe(OH)2 (s)     In the balanced equation, 3 OH- are present on the product side.     In the balanced equation, 5 molecules of water are present on the reagent side.     In the balanced equation, 4 molecules of water are present on the product side.     In the balanced equation, 5 molecules of water are present on the product side.     In the balanced equation, 3 OH- are present on the reagent side.     In the balanced equation, 4 molecules of water are present on the reagent side.