Question

You are given a 100.0 mL buffer that is 0.50 M HClO and 0.76 M in NaClO (Ka for HClO= 3.5x10^-8). What would the pH of the buffer solution change to if we added 10.0 mL 1.00 M HCl?

Answer 1

Buffer solution is a solution which resist the change in pH.

Molarity is number of moles of solute present in one litre of solution and is denoted by M

M = $\frac{Number of moles of solute *1000}{Volume of the solution in mL}$

$Number of moles of solute= \frac{M* Volume of solution in mL}{1000}$

This can be solved by two ways.

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clo + Hclo t Hor Adibom Gec O-06 Epuilibn 0-066 No-d mde,Hod o-06 mas Naodl o066 No Co.o6) ac) 46 + P - 46004ly 7.501 = S y + 4e0 clo mihal O-O76 Addihan a-0 final O066 O-06X 1000 0-545M O.066X1000 ito 746410910-6 JAS 46+hs11 -7-5