step 2) trial #1 mass of solid standard (KHP, potassium hydrogen phthalate) used = 0.100g; trial 1 equivalence point = 35.32 mL
step 5) mass of unknown (mixture of KHP and NaOH) = 1.5389g; trial #1 equivalence point = 10.50 mL
find requested weight percent
What happens in step 2) Use a convenient size flask and prepare an aqueous solution containing a known mass of KHP that will react with an estimated 25 mL of the unstandardized NaOH solution. (the flask will be a 100 mL volumetric flask)
What happens in step 5) Your unknown solid is a mixture of KHP and NaCl. Record the mass of the unknown and place it in a 100 mL volumetric flask. Dissolve your unknown in DI water then dilute to the mark. Sonication will speed dissolution. Perform four 25 mL titrations of the unknown solution with your standardized NaOH. On your first titration of the unknown, you may want to get a "rough" titration to get an idea where the endpoint lies. Calculate the weight percent of KHP in your unknown solid.
How to I find the weight percent given the above information (the equivalence point and masses obtained)?
step 2) trial #1 mass of solid standard (KHP, potassium hydrogen phthalate) used = 0.100g; trial...
A student weighs a sample of potassium hydrogen phthalate (KHP) to prepare a primary standard for a titration. She later discovers that the KHP was contaminated with sugar. To determine the amount of KHP in the mixture, she takes 5.942 g of the mixture and make a 100.0 mL solution. The student then titrates 10.00 mL of this solution with a 0.1491 M sodium hydroxide solution. She finds that 13.12 mL of the NaOH solution is needed to reach the...
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...
NaOH was standardized by titration against a standard acidic solution of potassium hydrogen phthalate (KHP). 0.4798 g of KHP were dissolved in 100 ml of water to prepare the standard KHP solution. a) What is the molar mass of KHP? (you need to look up its formula and calculate its molar mass from the periodic table). b) If 45.22 ml of sodium hydroxide were required to neutralize the KHP solution, what is the molarity of NaOH?
Potassium hydrogen phthalate, abbreviated KHP, is used to standardize NaOH solutions. A standard KHP solution is made by dissolving 2.12 grams of KHP in 100.00 mL of water. The KHP solution is then titrated with NaOH solution. It takes 23.12 mL of NaOH to reach the endpoint. What is the concentration of the NaOH?
KHP, potassium hydrogen phthalate (KHCHO is often used to standardie basic solution used in titration. If a 0.855. sample or KHP requires 31.44 ml of a KOR solution to fully realize it, what is the (KOH) in the solution? The reaction is KHC.H.O. KOHK C HO H O . 2. The KOH solution standardized above is used to titrate a 20.00-ml sample of sulfuric acid (H,SO.) solution of unknown concentration. Determine (H.SO.) for the unknown acid solution if 41.27 mL...
6. Potassium hydrogen phthalate (KHP, KHC8H4O4) is also a good primary standard. 20 mL of NaOH was titrated with 0.600 M KHC8H4O4 solution. The data was graphed and the equivalence point was found when 15.5 mL of the standard 0.600 M KHP solution was added. The reaction equation is: a. What is the molar ratio of NaOH:KHC8H4O4? b. What is the molarity of the NaOH solution?
Potassium hydrogen phthalate (KHP) is used to standardize sodium hydroxide. If 15.18 mL of NaOH(aq) is required to titrate 0.5614 g KHP to the equivalence point, what is the concentration of the NaOH(aq)? (The molar mass of KHP = 204.2 g/mol) HCH,0, (aq) + OH (aq) SCH,02 (aq) + H,0(1)
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...
The following data were collected during the titration of a solid sample of potassium acid phthalate ("KHP") with a solution of sodium hydroxide. The NaOH solution was added to the KHP from a buret. From the experiment data below, calculate the molarity of the NaOH solution. Data: Molar Mass of potassium acid phthalate= 204.23g/mol Mass of weighing bottle plus KHP= 23.4061 mL Mass of weighing bottle= 22.0515 g Initial buret reading= 0.20 mL Final buret reading= 39.13 mL
Materials: NaOH MW = 40 g/mL, KHP - potassium hydrogen phthalate, KHC8H404, MW = 204.23 g/mol. Acetic acid, HC2H302, MW = 60.05 g/mol Part 1: Standardization of NaOH Assume 0.951 g of KHP is weighed and transferred to a 250 mL Erlenmeyer flask. Approximately 50 ml water is added to dissolve the KHP. Note that the exact volume of water is not important because you only need to know the exact number of moles of KHP that will react with...