Students performing a similar analysis to your lab made several mistakes in their experiments. Explain how each error affected the calculated Molarity of the NaOH solution. Hint: start with deciding how the error will influence the quantities used in the equation for Molarity (Molarity = moles / Liter). Student A did not record the correct amount of KHP to use in the titration. The scale reading was 0.15 grams of KHP, but the student recorded the value as 0.10 grams of KHP. The student used the quantity 0.10 grams for the calculation.

See explanation

Explanation:

The reaction of NaOH and KHP is a neutralization reaction. The molarity of KHP is often calculated from the mass of KHP used to prepare the standard solution.

KHP is a slightly acidic substance. It is used as a primary standard for acid-base titrations because the solid is stable in air hence it is easy to weigh accurately. Also, the solid is neither hygroscopic nor deliquescent.

If student A recorded the amount of KHP used for the titration as 0.10g instead of 0.15g, then the molarity of NaOH calculated will be less than the actual the actual molarity of the NaOH.

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm