(a) A student carries out a titration to find the concentration of some sulfuric acid. The student finds that 25.00 cm of 0.0880 mol dm aqueous sodium hydroxide, NaOH, is neutralised by 17.60 cm of dilute sulfuric acid, H2SO4. H2SO4(aq) + 2NAOH(aq) → Na,SO,(aq) + 2H2O(1) (1) Calculate the amount, in moles, of NaOH used.

Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCI(aq), as described by the chemical equation MnO, (s) + 4 HCl(aq) MnCl, (aq) + 2 H,0(1) + Cl,(g) How much MnO,(s) should be added to excess HCI(aq) to obtain 145 mL Cl, (g) at 25 °C and 735 Torr? 1.097 mass of MnO, : Incorrect

To measure the amount of calcium carbonate (CaCO3) in a seashell, an analytical chemist crushes a 4.30 g sample of the shell to a fine powder and titrates it to the endpoint with 233. mL of 0.2700M hydrogen chloride (HCI) solution. The balanced chemical equation for the reaction is: 2HCl(aq) + CO3(aq) → H₂CO3(aq) + 2Cl(aq) 19 0 What kind of reaction is this? O precipitation O acid-base redox X olo If you said this was a precipitation reaction, enter the chemical formula of the precipitate. 0 Ar 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 CaCO3 in the sample. Be sure your answer has 3 significant digits. П 0 0% S ?

How many millilitres of 0.450 mol L−1 H2SO4(aq) are required to completely neutralize 46.7 mL of 0.930 mol L−1 KOH(aq) ? Hint: Write a balanced chemical equation for the reaction.   Give your answer in mL, accurate to three significant figures. Do not include units as part of your answer.

The concentration of SO32- in a solution is determined by titrating it with a 0.1464 M dichromate solution. The balanced net ionic equation for the reaction is: Cr₂O72-(aq) + 3SO32(aq) + 8H30*(aq) → 2Cr³+ (aq) + 3504²(aq) + 12H₂O(l) In one experiment, 23.91 mL of the 0.1464 M dichromate solution is required to react completely with 30.00 mL of the SO32- solution. Calculate the concentration of the SO3²- solution. M

For each of the following reactions, suggest two soluble ionic compounds that, when mixed together in water, result in the net ionic equation given: (a) 2 Ag+ (aq) + CO3²¯ (aq) → Ag₂CO3(s) (b) Mg²+ (aq) + 2 OH¯(aq) → Mg(OH)₂(s), the suspension present in milk of magnesia 3+ (c) 3 Ca³+ (aq) + 2 PO2 (aq) → Ca3(PO4)2(s), gypsum, a component of concrete

As shown in the following Figure, an aqueous solution of Nal is poured into an aqueous solution of Pb(NO3)2 which results in the formation of a yellow precipitate. Assuming stoichiometric amounts of Nal and Pb(NO3)2 are reacted, give the chemical formula of the yellow precipitate and the chemical formula of all molecules and/or ions that are present in the solution (You may use the solubility matrix to answer this question). (b)

A solution of permanganate is standardized by titration with oxalic acid, H₂C₂O4. To react completely with 1.000 × 10-³ mol of oxalic acid required 35.29 mL of permanganate solution. The unbalanced chemical equation for the reaction in acidic solution is MnO4 (aq) + H₂C₂O4 (aq) → →Mn²+ (aq) + CO2 (9) Determine the concentration of the permanganate solution in molarity. Concentration = M

Sodium hydroxide is extremely soluble in water. At a certain temperature, a saturated solution contains 539 g NaOH(s)539 g NaOH(s) per liter of solution. Calculate the molarity of this saturated NaOH(aq)NaOH(aq) solution.

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.