An aqueous solution of 0.1 M H2SO4(aq) is added to 0.1 M Na2S(aq) and is allowed to react. From the following, select all of the statements that are true.     The product of the reaction will have a colored supernatant     The product of the reaction will have a colorless supernatant     The reaction will produce water as a product     The reaction will produce a precipitate     The reaction will produce a gas     The reaction will result in an oxidation and/or reduction of one of the reactants

A copper penny dropped into a solution of nitric acid produces a mixture of nitrogen oxides. The following overall balanced reaction describes the formation of nitrogen monoxide, one of the products: 3 Cu(s)+8 H+(aq)+2 NO3−(aq) → 2 NO(g)+3 Cu2+(aq)+4 H2O(l) A.) Identify the Oxidant the the Reductant B.)Calculate E∘ for this reaction at 25 ∘C. C.) Calculate ΔG∘ for this reaction at 25 ∘C D.) Calculate the reaction potential at 25 ∘C when [NO3−]= 0.075 M, [Cu2+]= 0.0076 MM, [NO]= 0.010 MM, and the pH is 0.00.

the number of moles of Aluminum in 1.3741 g was calculated to be 0.051 moles and that the chemistry student weighed out.  For every mole of Aluminum that you start with, you can create one mole of Alum [KAl(SO4)2 ⋅12 H2O(s)].  What is the theoretical yield before drying the Alum precipitate?

The following skeletal oxidation-reduction reaction occurs under acidic conditions. Write the balanced OXIDATION half reaction. Co + Ag*Ag + Co²+ Products Reactants

Write the formation equation for X-(aq), MX(s), and M+(aq). Assume all atoms used are monoatomic solids in the standard state.

Give the concentrations of all ions in each of the following solutions. 50 M Co(NO3)2     0 M FeCl3     25M Ba(OH)2 (aq)

50 mL of a 1.067 M solution of HCI was diluted to 250 mL. The diluted HCI solution was then titrated with an unknown concentration of KOH. It is found that an average volume of 24.20 mL of KOH is required to reach an endpoint in a titration with 25.00 mL of the dilute acid solution. The equation for the reaction is; H(aq) + OH(aq) →→> H₂O (1) The concentration of KOH is 0.2205 M Calculate the concentration of the KOH in g/L (you will need to find the formula weight of KOH to do this) 15| ΑΣΦ ? g/L

A 0.25 M solution of magnesium nitrate is diluted to one half its original concentration. What is the total concentration of ions (magnesium ions AND nitrate ions) in the dilute solution? a) 0.125 M b) 0.25 M c) 0.375 M d) 0.50 M e) 0.75 M

A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach the endpoint, a total of 26.0 mL of HNO₃ was required. Write the balanced chemical equation based on the following description: aqueous calcium hydroxide reacts with aqueous nitric acid to produce the aqueous calcium nitrate and liquid water.

Write the balanced net ionic equation for the precipitation of lead (II) hydroxide from aqueous solution:  write the balanced net ionic equation for the precipitation of chromium (iii) sulfide from aquesous solution: