Answer
0.1191M
Explanation
The reaction between KHP and NaOH is 1:1molar
KHP(aq)+ NaOH(aq) -----> NaKHP(aq) + H2O(l)
mole = mass/molar mass
moles of KHP = 0.400g /204.22g/mol = 0.001959mol
0.001959moles of KHP react with 0.001959moles of NaOH
moles of NaOH present in the 16.45ml of NaOH solution = 0.001959mol
molarity = number of moles of solute per liter of solution
molarity of NaOH = (0.001959mol/16.45ml) ×1000ml = 0.1191M
formula for KHP is KC8H5O4 A beaker containing 0.400 g KHP was titrated with NaOH solution....
Question 6 Status: Tres remaining 3 1 Points possible: 1.00 A beaker containing 0.400 g KHP was titrated with NaOH solution. The pale pink end point was reached after 18.55 mL of NAOH solution was dispensed. What is the molarity of the NaOH solution? Answer: CHECK
Question 6 Status: Tries remaining: 3 Points possible: 1.00 A beaker containing 0.400 g KHP was titrated with NaOH solution. The pale pink end point was reached after 19.55 mL of NaOH solution was dispensed. What is the molarity of the NaOH solution? Answer:
Question 5 Status: Tries remaining: 3 Points possible: 1.00 Calculate the molarity of a solution prepared by dissolving 0.187 g of KHP in enough water to make 125 mL of solution. The formula of KHP is KC H504 Answer: CHECK Question 6 Status: Tries remaining: 3 1 Points possible: 1.00 A beaker containing 0.400 g KHP was titrated with NaOH solution. The pale pink end point was reached after 18.55 mL of NaOH solution was dispensed. What is the molarity...
Standardization of NaOH solution experiment: A 0.75 g sample of pure acid KHP was titrated to phenolphthalein endpoint using 45.34 ml NaOH of unknown concentration. The formula weight of pure KHP is 204.22g/mol. Write the chemical equation for the neutralization reaction, indicate the color change of the indicator at the endpoint, and calculate molarity of the NaOH solution. Show your work. 1. Chemical equation ------------- 2. Endpoint color change ---- 3. NaOH molarity --------- Determine percent purity of impure KHP...
If 35.22 mL of NaOH solution completely neutralizes a solution containing 0.544 g of KHP, what is the molarity of the NaOH solution?
1. A solution of sodium hydroxide (NaOH) was standardized against potassium hydrogen phthalate (KHP). A known mass of KHP was titrated with the NaOH solution until a light pink color appeared using phenolpthalein indicator. Using the volume of NaOH required to neutralize KHP and the number of moles of KHP titrated, the concentration of the NaOH solution was calculated. Molecular formula of Potassium hydrogen phthalate: HKC8H404 Mass of KHP used for standardization (g) 0.5100 Volume of NaOH required to neutralize...
1. A solution of sodium hydroxide (NaOH) was standardized against potassium hydrogen phthalate (KHP). A known mass of KHP was titrated with the NaOH solution until a light pink color appeared using phenolpthalein indicator. Using the volume of NaOH required to neutralize KHP and the number of moles of KHP titrated, the concentration of the NaOH solution was calculated. Molecular formula of Potassium hydrogen phthalate: HKC8H404 Mass of KHP used for standardization (g) 0.5306 Volume of NaOH required to neutralize...
A 1.413-g sample of KHP takes 19.43 mL of a NaOH solution to titrate it to a phenolphthalein end point. What is the molarity of the NaOH solution? The molar mass of KHP is 204.2g/mol.
An unknown sample (0.6855 g) containing KHP is titrated to the equivalence point with 9.7 mL of 0.0789 M NaOH. a) How many moles of KHP are present? b) How many grams of KHP are present (molecular weight of KHP = 204.23 g/mol)? c) What is the percent KHP in the sample?
A solution of NaOH is standardized with potassium acid phthalate (KHP), KHC8H8O4, molar mass = 204 g/mol. If 2.550 g of KHP is titrated with 54.50 mL of the NaOH solution, what is the molarity of NaOH?