Question

Calculate the molar concentration of an NaOH solution that required 15.81 mL to com- pletely neutralize 0.509 g of KHP (Remember that the "P" in KHP does not mean phos- phorus. See the molecular structure and molar mass of KHP given earlier in the lab.) 3. KHP(s)+NaOH(aq) -NaKP(aq) +H,O(e) Calculate the mass of KHP that will react completely with 25.00 mL of 0.1750 M NaOH 4. 5 Write the balanced equation for the reaction that occurs when aqueous HCl is added to solid CaCO, and the solution is heated. 6. Calculate the mass of solid NaOH needed to prepare 250.0 mL of 0.1000 M NaOH solu- tion. 4 CHM 210 Lab 11

Any help would be great. thank you

Answer 1

Question 3

Mass of KHP = 0.509 gm

Molar mass of KHP = 204.22 g/mol

Moles of KHP = 0.509 gm/ 204.22 g/mol = 0.002492 Moles

Moles of NaOH reacted = 0.002492 Moles

VOlume of NaOH = 15.81 ml

Molar concentration of NaOH = 0.002492 x 1000 / 15.81 = 0.1576 M

Question 4

Concentration of NaOH = 0.1750 M

VOlume of NaOH = 25 ml

Moles of NaOH reacted = 0.1750 x 25 /1000 = 0.004375‬ Moles

Moles of KHP reacted =  0.004375‬ Moles

Mass of KHP reacted =   0.004375‬ Moles x 204.22 gm/mol = 0.8935 gm

Question 5

Balanced equation:
2 HCl (aq) + CaCO₃ (s) ====> CaCl₂ (s) + H₂O (l) + CO₂ (aq)

Question 6

Mass of solid NaOH required = 250 x 0.1 x 40 /1000 = 1 gm