Question

Calculate the pH change that results when 15 mL of 2.6 M HCl is added to 600. mL of each of the following solutions. (See the appendix.) (a) pure water    (b) 0.10 M CH3COO? (c) 0.10 M CH3COOH (d) a solution that is 0.10 M in each CH3COO? and CH3COOH. Table 3 An Acid-base table Acid Name ConjugateAcid Ka pKa Conjugate Base Base Name perchloric acid HClO4 >>1 < 0 ClO41- perchlorate ion hydrohalic acid HX (X=I,Br,Cl) >>1 < 0 X1- halide ion sulfuric acid H2SO4 >>1 < 0 HSO41- hydrogen sulfate ion nitric acid HNO3 >>1 < 0 NO31- nitrate ion hydronium ion H3O1+ 1.0 0.00 H2O water iodic acid HIO3 0.17 0.77 IO31- iodate ion oxalic acid H2C2O4 5.9 x 10-2 1.23 HC2O41- hydrogen oxalate ion sulfurous acid H2SO3 1.5 x 10-2 1.82 HSO31- hydrogen sulfite ion hydrogen sulfate ion HSO41- 1.2 x 10-2 1.92 SO42- sulfate ion phosphoric acid H3PO4 7.5 x 10-3 2.12 H2PO41- dihydrogen phosphate ion hydrofluoric acid HF 7.2 x 10-4 3.14 F1- fluoride ion nitrous acid HNO2 4.0 x 10-4 3.40 NO21- nitrite ion lactic acid HC3H5O3 6.4 x 10-5 3.85 C3H5O31- lactate ion formic acid HCHO2 1.8 x 10-4 3.74 CHO21- formate ion hydrogen oxalate ion HC2O41- 6.4 x 10-5 4.19 C2O42- oxalate ion hydrazoic acid HN3 1.9 x 10-5 4.72 N31- azide ion acetic acid HC2H3O2 1.8 x 10-5 4.74 C2H3O21- acetate ion carbonic acid H2CO3 4.3 x 10-7 6.37 HCO31- hydrogen carbonate ion hydrogen sulfite ion HSO31- 1.0 x 10-7 7.00 SO32- sulfite ion hydrosulfuric acid H2S 1.0 x 10-7 7.00 HS1- hydrogen sulfide ion dihydrogen phosphate ion H2PO41- 6.2 x 10-8 7.21 HPO42- hydrogen phosphate ion hypochlorous acid HClO 3.5 x 10-8 7.46 ClO1- hypochlorite ion ammonium ion NH41+ 5.6 x 10-10 9.25 NH3 ammonia hydrocyanic acid HCN 4.0 x 10-10 9.40 CN1- cyanide ion hydrogen carbonate ion HCO31- 4.7 x 10-11 10.33 CO32- carbonate ion hydrogen phosphate ion HPO42- 4.8 x 10-13 12.32 PO43- phosphate ion hydrogen sulfide ion HS1- 1.3 x 10-13 12.89 S2- sulfide ion water H2O 1.0 x 10-14 14.00 OH1- hydroxide ion ammonia NH3 <<10-14 NH21- amide ion hydroxide ion OH1- <<10-14 O2- oxide ion

Answer 1

Solution :-

Given data

15 ml 2.6 M HCl

Part a) 15 ml 2.6 M HCl added to 600 ml pure water

Lets first calculate final concentration of the HCl after mixing the 15 ml 2.6 M HCl with 600 ml pure water

After mixing final volume is = 15 ml + 600 ml = 615 ml

Formula to calculate final concentration is as follows

M1V1=M2V2

Where M1 = initial concentration

V1= initial volume

M2= Final concentration

V2= final volume

Lets put the values in the formula and solve for M2

M1V1=M2V2

2.6 M * 15 ml = M2 * 615 ml

M2 = (2.6 M * 15 ml )/615 ml

M2 = 0.0634 M

HCl is the strong acid so it dissociate completely therefore concentration of the H⁺ is same as concentration of HCl that is 0.0634 M

Lets calculate pH using this H⁺ concentration

Formula to calculate pH is as follows

pH= - log[H⁺]

pH= - log [ 0.0634]

pH= 1.20

part b) 15 ml 2.6 M HCl added to 600 ml 0.10 M CH3COO-

reaction equation is as follows

HCl + CH3COO-