Question

1.)Assuming equal concentrations, rank these solutions by pH. Ca(OH)2(aq) ,NH3(aq) , HI(aq), NaOH(aq) , HF(aq)

2.) Write the chemical equation for the reaction of carbonic acid (H2CO3) with water.

3.) Calculate either [H3O ] or [OH–] for the solutions below at 25 °C.

a.) [OH-]= 3.33*10^-7 M [H3O+]=

b.) [H3O+]=9.93*10^-9 M [OH-]=

c.) [H3O+]=.000571 M [OH-]=

4.) Complete these Brønsted-Lowry reactions. HCO-+H+ the 3 is right belowe the negative sign and then after the H+ arrows are facing left and right.

3

HCO- + OH-----> arrows are also facing both directions and 3 is below negative sign.

3

5.) Complete this Brønsted-Lowry reaction, placing each product by its appropriate label. HPO2- + F- which one is acid and which one is base?

4

6.)A monoprotic acid, HA, is dissolved in water: The equilibrium concentrations of the reactants and products are [HA] = 0.140 M [H ] = 4.00 × 10–4 M [A–] = 4.00 × 10–4 M Calculate the value of pKa for the acid HA. calculate the value of pka

7.)A monoprotic acid, HA, is dissolved in water: The equilibrium concentrations of the reactants and products are [HA] = 0.100 M [H3O ] = 2.00 × 10–4 M [A–] = 2.00 × 10–4 M Calculate the Ka value for the acid HA.

Answer 1

Post one more question to get the remaining answers

1) Ca(OH)2 and NaOH are strong bases and hence will dissociate completely in the solution

NH3 is a weak base whereas HF and HI are strong acid

pH order will be Ca(OH)2 > NaOH > NH3 > HF > HI

2) H2CO3 + H2O ------ HCO3(-) + H3O+

HCO3- + H2O ----- CO3(2-) + H3O+

H2CO3 is diprotic acid

3)

a) [H3O+][OH-] = 10^(-14)

[H3O+] = 10^(-14)/(3.33 * 10^(-7)) = 3 * 10^(-8) M

b) [H3O+][OH-] = 10^(-14)

[OH-] = 10^(-14)/(9.93 * 10^(-9)) = 1.007 * 10^(-6) M

c) [H3O+][OH-] = 10^(-14)

[OH-] = 10^(-14)/(0.000571) = 1.751 * 10^(-11) M