Can adding baking soda (a base) to a lotion raise the pH

The lotion in question is a glycolic acid lotion, but the company sells the lotion at a dangerous pH of 1.

http://www.texasnaturalsupply.com/produc…

Can baking soda effectively raise the pH to 3 or 4? If so, how much NaHCO3 would you guesstimate to be necessary for 8 oz and 28 oz of lotion (at a pH of 1).

Thanks in advance.

This is an interesting problem in unit conversion.

General facts : Use Henderson-Hasalbalch equation for making a buffer solution.

pH = pKa + log([A-]/[HA])

other facts:
pKa of glycolic acid is 3.83, which is in the range of 3 to 4 as desired.
Web site from Texas Natural Supply says glycolic solution was 15%, which equals 15g/100ml.
Molecular wt of Glycolic acid is 76.05 g/mole.
Molecular wt of NaHCO3 is 84.01 g/mole.
1 oz. = 29.574 ml.

So plugging this into the HH equation, we see that if the A- form has the same molar concentration as the HA form then the pH of the resulting solution will equal the pKa, which in this case is 3.83, which is in the desired range.

So the concentration of the HA form (glycolic acid) =
(15g/100ml)(1mol/76.0g)(8 oz)(29.574 ml/ 1oz)= 0.467 moles glycolic acid in 8 oz of cream.

add (0.467 mole) (84.10g/mol) = 39.2030 g, (1.38 oz) NaHCO3 into 8 Oz jar and stir to mix,

add (0.467 mole)(84.10g/mol)( 28/8) = 137.212 g, (4.84 oz) NaHCO3 into 28 Oz jar and stir to mix.

I don't know if the bicarbonate will mix easily with the glycolic acid cream, but the calculated grams or ounces are correct.