1. Solid NH4NO3 dissolves in water and then reacts with KOH (aq). The container releases a smell as the reaction proceeds. (a) Write the acid-base reaction products for this reaction. (b) Write the decomposition reaction that happens immediately after the acid-base reaction that is responsible for the smell observed.

A 0.124 M NaOH(aq) solution was used to titrate 20.00 mL of an acetic acid (CH3COOH) solution that has an unknown concentration. The equivalence point is reached after adding 15.34 mL of NaOH(aq). a) Write out the complete balanced equation for the reaction that occurs in this titration. b) How man moles of NaOH were added to the acetic acid solution? c) How many moles of acetic acid were in the original 20.00 mL solution? d) What was the concentration of acetic acid in the orignial 20.00 mL solution?

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)

When sodium acetate, CH3COONa(s), is added to CH3COOH (aq), why does the pH of the solution increase?

(a) The sodium ion did not take part in this chemical reaction. What do we call such an ion? (b) Draw a simple diagram which shows how the sodium ion mixes with water in solution. What do we call this physical process?

Much of the sulfur used in the United States comes from the hydrogen sulfide contaminant that makes "sour" natural gas smell bad. Hydrogen sulfide is separated from the other components of natural gas mostly by taking advantage of its acid-base reaction with aqueous ethanolamine: HO(CH,),NH,(aq)+H,S(g) → HO(CH,),NH,(aq)+HS (aq) Suppose an engineer decides to study the rate of this reaction. She prepares four reaction vessels with 167.6 mL of ethanolamine solution and 20.9 g of hydrogen sulfide gas each. The volume and temperature of each vessel is shown in the table below. Arrange the reaction vessels in decreasing order of initial rate of reaction. In other words, select a "1" next to the vessel in which the engineer can reasonably expect the initial rate of reaction to be highest, a "2" next to the vessel in which the initial rate of reaction would be next highest, and so on. vessel volume temperature A B C D 5.0 L 5.0 L 5.0 L 5.0 L 49, °C 48. °C 51. °C 50. °C X initial rate of…

By titration, it is found that 39.1 mL of 0.161 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.

Give the answers that should be filled in the blanks below: Acetic acid solution: pH = 5.80; (a) [H+] =         M; (b) [OH-] =          M Ammonia solution: [H+] = 5.90 x 10-9 M; (c) pH =           ; (d) pOH =

How many millilitres of 0.590 mol L−1 H2SO4(aq) are required to completely neutralize 28.1 mL of 0.570 mol L−1 KOH(aq) ? Hint: Write a balanced chemical equation for the reaction.   Give your answer in mL, accurate to three significant figures

The following chemical reaction takes place in aqueous solution: CuBr2(aq)+2KOH(aq)→CuOH2(s)+2KBr(aq).Write the net ionic equation for this reaction.