1) The color of bromocresol green indicator is??? when pH < 4, green when pH 4- 5.3 and ???? in pH > 5.3.

2)(A) A student performed the freezing point depression experiment according to directions but mistakenly recorded the mass of lauric acid as 8.300 g instead of 8.003 g. The calculated molar mass of the unknown acid will be ___________ than the true value, because the mass of lauric acid appears in the denominator of the unknown acid's molecular weight determination

Bromocresol green indicator turns from yellow in acid to blue in base.

I am troubled by this question as I indicated in an answer to the same question yesterday. The mass of the lauric acid may appear in the denominator or it may appear another place depending upon how the equations are set up. However, since grams/molar mass = mols, then a larger number for grams will result in a larger number for mols and that will give high results.

1) The color of bromocresol green indicator is yellow when pH is less than 4, green when pH is between 4 and 5.3, and blue in pH greater than 5.3.

2) (A) Since the mass of lauric acid appears in the denominator of the unknown acid's molecular weight determination, an increase in the recorded mass of lauric acid will result in a calculated molar mass of the unknown acid that is higher than the true value.

1) The color of bromocresol green indicator is yellow when the pH is less than 4, green when the pH is between 4 and 5.3, and blue when the pH is greater than 5.3.

To find the answer to this question, you can refer to a color chart or consult a reliable source that provides information about the color changes of bromocresol green indicator at different pH levels.

2)(A) In the freezing point depression experiment, the mass of lauric acid is mistakenly recorded as 8.300 g instead of 8.003 g. This error in mass will lead to an overestimation of the molar mass of the unknown acid.

To calculate the molar mass of the unknown acid, the formula for freezing point depression can be used. The formula is:

ΔT = Kf * m

ΔT is the change in freezing point temperature, Kf is the cryoscopic constant for the solvent, and m is the molality of the solute.

Since the mass of lauric acid appears in the denominator of the molecular weight determination of the unknown acid, a higher recorded mass will result in a smaller molality value. This leads to a larger value for the calculated molar mass of the unknown acid, compared to the true value. Therefore, the calculated molar mass will be higher than the true value.