chemistry
1.
2.
Complete the following table:
| [H3O+] mol.dm-3 | 3.6 x 10-3 | | | | |
| [HO-] mol.dm-3 | | 3.6 x 10-3 | | 6.3 x 10-5 | |
| pH | | | 10.4 | | 7.0 |
1.
2.
Calculate the pH of a solution of acetic acid where [CH3COOH] = 0.05 mol.dm-3. (pKa CH3COOH/CH3COO- = 4.74)
Original post by hoprovenia
1.
Calculate the pH of a solution of acetic acid where [CH3COOH] = 0.05 mol.dm-3. (pKa CH3COOH/CH3COO- = 4.74)
do 10-pka to find the ka value, then rearrange the formula
ka= [H+]2/[HA] to find H+ and then do -log[H+] to find ph to 2 decimal places.
Gosh they're dumbing down these Masters courses aren't they
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