1.)Assuming equal concentrations, rank these solutions by pH. Ca(OH)2(aq) ,NH3(a
ID: 944492 • Letter: 1
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.
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HCO- + OH-----> arrows are also facing both directions and 3 is below negative sign.
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5.) Complete this Brønsted-Lowry reaction, placing each product by its appropriate label. HPO2- + F- which one is acid and which one is base?
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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.
Explanation / Answer
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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
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