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Calculate the mass of each of the following acids that would be needed to prepare 100...
A solution of NaOH is standardized with potassium acid phthalate (KHP), KHC8H8O4, molar mass = 204...
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?
1. A solution of sodium hydroxide (NaOH) was standardized against potassium hydrogen phthalate (KHP). A known...
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...
3. 0.7253 g sample containing an unknown weak acid HA was dissolved in 50 mL water...
3. 0.7253 g sample containing an unknown weak acid HA was dissolved in 50 mL water and titrated against 0.1555 M NaOH, requiring 48.11 mL to of NaOH to reach the end-point. During the titration reaction, the pH of the solution is 3.77 when half of the HA is neutralized and the equivalence-point pH is 8.33. (a) State two ways to standardize the NaOH used in the titration. (b) Suggest and explain an indicator that can be used in the...
How do I calculate the ionization constant for acetic acid from the measured pH of the acedic aci...
How do I calculate the ionization
constant for acetic acid from the measured pH of the acedic acid
samples?
Data and Calculations 1. Measurement of pH and fitration of acetfic acid solution Concentration of standardized NaOH titrant Mass concentration of acetic acid-aao Trial 3 Trial 2 Trial 1 Measured pht of the acetic acid solution Mass of acetic acid solution taken for titration. Initial buret reading of NaOH titrant Final buret reading of NaOH titrant Net volume of NaOH Millimoles...
Mass potassium hydrogen phthalate: .459 g Concentration NaOH solution: .10 M Strong Base titrated...
Mass potassium hydrogen phthalate: .459 g
Concentration NaOH solution: .10 M
Strong Base titrated into weak acid
1. ml base added at equivalence point?
2. ml base added at half-neutralization point 3. moles acid left unreacted at half-neutralization point 3 a. moles salt present at half-neutralization point b. moles of anion of salt present at half-neutralization point 5. ratio of moles of anion to moles of unreacted acid at half-neutralization point 6. . pKa of potassium hydrogen phthalate b. explanation...
50.0 mL sample of the weak acid the concentration of the weak acid = 0.15 M...
50.0 mL sample of the weak acid
the concentration of the weak acid = 0.15 M
25 mL of the week acid into 100 mL beaker
titrated this solution of 0.21 M NaOH
moles of weak acid = 3.75*10^-3
moles of NaOH = moles of week acid
c) How many milliliters of the NaOH are required to neutralize the sample of weak acid? d) How many moles of NaOH have been added at one half of the volume in part...
millimoles of NaOH titrant Chemical Equilibria: K, of a Weak Monoprotic Acid Report Form Name: Partner's...
millimoles of NaOH titrant
Chemical Equilibria: K, of a Weak Monoprotic Acid Report Form Name: Partner's Name: (if any) Lab Section MWITTHM-TH (Circle) Data and Calculations 1. Measurement of pH and titration of acetic acid solution Concentration of standardized NaOH titrant 0.1054 Mass concentration of acetic acid 2.40 - mol/L Trial 3 Measured pH of the acetic acid solution Mass of acetic acid solution taken for titration Trial 1 3.09 20.16 0 11.4 Trial 2 3.32 30.06 Initial buret reading...
2. Calculate the mass of solid sodium hydroxide needed to prepare 300 mL of 0.1 M...
2. Calculate the mass of solid sodium hydroxide needed to prepare 300 mL of 0.1 M sodium hydroxide. Note: Be sure to include this mass in the procedure for Part C. 3. A 0.6250 g sample of KHP (204.2 g/mol), dissolved in 50 mL water, required 28.50 mL of sodium hydroxide to reach the end point. What is the concentration of the sodium hydroxide solution? 4. A 25.00 mL sample of hydrochloric acid was titrated using the same sodium hydroxide...
please help After answering these questions, enter your answers in Bb The system has been setup for 2 attempts. If f...
please help
After answering these questions, enter your answers in Bb The system has been setup for 2 attempts. If for any reason, the system fails, write your answers on this page, tear out the page from the manual and give this to your TA before prelab lecture starts. You are allowed up to two paper submission per quarter. 1. What is the proper reading of the buret shown? Question 1 answers 20.5 ml 19.44 ml 19.5 ml 19.6 mL...
Each group of students should prepare 100 mL of ONE of the following PAIRS of buffers...
Each group of students should prepare 100 mL of ONE of the following PAIRS of buffers 2. Phosphate buffer a. 100 mM potassium-phosphate, pH 5.0 b. 100 mM potassium-phosphate, pH 7.0 To prepare 100 mL of 100 mM phosphate buffers by titrating the monobasic form with base, first calculate how much KH2PO4 you need. Dissolve this amount in 50 mL of water. Using the Henderson-Hasselbalch equation, calculate how much 1 M NaOH should be required to achieve the desired pH...
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...
How do I calculate the ionization
constant for acetic acid from the measured pH of the acedic acid
samples?
Data and Calculations 1. Measurement of pH and fitration of acetfic acid solution Concentration of standardized NaOH titrant Mass concentration of acetic acid-aao Trial 3 Trial 2 Trial 1 Measured pht of the acetic acid solution Mass of acetic acid solution taken for titration. Initial buret reading of NaOH titrant Final buret reading of NaOH titrant Net volume of NaOH Millimoles...
Mass potassium hydrogen phthalate: .459 g
Concentration NaOH solution: .10 M
Strong Base titrated into weak acid
1. ml base added at equivalence point?
2. ml base added at half-neutralization point 3. moles acid left unreacted at half-neutralization point 3 a. moles salt present at half-neutralization point b. moles of anion of salt present at half-neutralization point 5. ratio of moles of anion to moles of unreacted acid at half-neutralization point 6. . pKa of potassium hydrogen phthalate b. explanation...
50.0 mL sample of the weak acid
the concentration of the weak acid = 0.15 M
25 mL of the week acid into 100 mL beaker
titrated this solution of 0.21 M NaOH
moles of weak acid = 3.75*10^-3
moles of NaOH = moles of week acid
c) How many milliliters of the NaOH are required to neutralize the sample of weak acid? d) How many moles of NaOH have been added at one half of the volume in part...
millimoles of NaOH titrant
Chemical Equilibria: K, of a Weak Monoprotic Acid Report Form Name: Partner's Name: (if any) Lab Section MWITTHM-TH (Circle) Data and Calculations 1. Measurement of pH and titration of acetic acid solution Concentration of standardized NaOH titrant 0.1054 Mass concentration of acetic acid 2.40 - mol/L Trial 3 Measured pH of the acetic acid solution Mass of acetic acid solution taken for titration Trial 1 3.09 20.16 0 11.4 Trial 2 3.32 30.06 Initial buret reading...
2. Calculate the mass of solid sodium hydroxide needed to prepare 300 mL of 0.1 M sodium hydroxide. Note: Be sure to include this mass in the procedure for Part C. 3. A 0.6250 g sample of KHP (204.2 g/mol), dissolved in 50 mL water, required 28.50 mL of sodium hydroxide to reach the end point. What is the concentration of the sodium hydroxide solution? 4. A 25.00 mL sample of hydrochloric acid was titrated using the same sodium hydroxide...
please help
After answering these questions, enter your answers in Bb The system has been setup for 2 attempts. If for any reason, the system fails, write your answers on this page, tear out the page from the manual and give this to your TA before prelab lecture starts. You are allowed up to two paper submission per quarter. 1. What is the proper reading of the buret shown? Question 1 answers 20.5 ml 19.44 ml 19.5 ml 19.6 mL...
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