Coke has a pH of 2.6. Assuming that the acidity of the Coke is due solely...
Coke has a pH of 2.6. Assuming that the acidity of the Coke is due solely to carbonic acid and the density of Coke is 1.11g/mL, then the carbonic acid concentration calculates to be 0.86% by mass in Coke. What is the volume of 0.02M sodium hydroxide required to neutralize an entire can of Coke which is 374g? The molar mass is carbonic acid is 62g/m.
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Coke has a pH of 2.6. Assuming that the acidity of the Coke is
due solely...
Need help with this prelab please Experiment 10 Prelaboratory Assignment Vinegar Analysis Lolo Sec. Name...
Need
help with this prelab please
Experiment 10 Prelaboratory Assignment Vinegar Analysis Lolo Sec. Name I. Asunning the to of a 59. acetic acid by mass sclution is 10 Desk No. 25.0 ml. of density 0.10 M NaoH Also record desemnine volume of aceic acid" dhis calculation your Report Sheet A chemist often uses a white card with a black mark to aid in reading the meniscus of a technique make the reading more clear liquid. How does this b....
3. For the n=5 to n=2 transition: E = in nm = in Å = Color...
3. For the n=5 to n=2 transition: E = in nm = in Å = Color of corresponding line in the hydrogen spectrum: b. Calculate the molar concentration of the hydrochloric acid if 35.18 mL of hydrochlo- ric acid was required to neutralize 0.450 g of sodium bicarbonate to a phenolphthalein end point. C. Calculate the mass percent concentration of hydrochloric acid using the molar con- centration calculated in part band assuming the density of the solution is 1.01 g/mL....
What volume of a 0.333 M hydrobromic acid solution is required to neutralize 24.7 mL of...
What volume of a 0.333 M hydrobromic acid solution is required to neutralize 24.7 mL of a 0.152 M barium hydroxide solution? mL hydrobromic acid Submit Answer Retry Entire Group 6 more group attempts remaining What volume of a 0.207 M hydroiodic acid solution is required to neutralize 24.3 mL of a 0.183 M potassium hydroxide solution? mL hydroiodic acid Submit Answer Retry Entire Group 6 more group attempts remaining What volume of a 0.161 M sodium hydroxide solution is...
Please help, I'm so confused!!!! This is due wednesday night!!! i'm gonna fail :(((( pH of...
Please help, I'm so confused!!!! This is due wednesday night!!!
i'm gonna fail :((((
pH of Buffer Solutions Procedure: Acetic Acid-Sodium Acetate Buffer (pKa acetic acid = 4.75) Weigh about 3.5 g of Na2C2H302 3H2O, record the exact mass, and add to a 250 ml beaker. Measure exactly 8.8 mL of 3.0 M acetic acid (use 10 mL grad cylinder) and add to the beaker containing the sodium acetate. • Measure exactly 55.6 mL of distilled water and add to...
3) Assume that the pH of rain is 4.0 and that the acidity is due entirely...
3) Assume that the pH of rain is 4.0 and that the acidity is due entirely to HNO3(a poor assumption---typically, H2SO4 is a greater contributor to acid rain than HNO3). Calculate the mass of the primary pollutant NO that was required to acidify 1 L of rain. Assume that each mole of NO is oxidized to one mole of HNO3.
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...
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...
A buffer with pH = 10.15 is to be prepared by addition solid sodium hydrogen carbonate...
A buffer with pH = 10.15 is to be prepared by addition solid sodium hydrogen carbonate to 1.00 L of 0.300 M sodium carbonate. What mass is required assuming the volume does not change? For carbonic acid, Ka1 = 4.45 x 10-7 and Ka2 = 5.69 x 10-11
I would like help understanding these questions. Thank you for your time! Acids/Bases 1. Calculate the...
I would like help understanding these questions.
Thank you for your time!
Acids/Bases 1. Calculate the volume (in mL) of a 1.75 M KOH solution required to completely titrate (neutralize) 16.0 mL of a 3.00 M phosphoric acid solution. 2. Calculate the concentration of a sodium hydroxide solution that required 43.40 mL to completely titrate 26.50 mL of a 0.350 M oxalic acid (H2C2O4) solution. 3. Calculate the pH of the following: (a) a solution containing a hydronium concentration of...
Due ; Went so CIVE.3620 Homework: Environmental Chemistrye hem (Note: A similar problem was previously a...
Due ; Went so CIVE.3620 Homework: Environmental Chemistrye hem (Note: A similar problem was previously a 20/100 point question on an hour exam.) 8. Strong bas es and strong acids completely dissociate in solution. e ttration of strong acids and bases the following neutralization reaction occurs: H OH strong base. H2O. Nitric acid and sodium hydroxide are a strong acid and a A solution cont sodium hydroxide (NaOH) th taining nitric acid (HNO,) is to be used in the neutralization...
Need
help with this prelab please
Experiment 10 Prelaboratory Assignment Vinegar Analysis Lolo Sec. Name I. Asunning the to of a 59. acetic acid by mass sclution is 10 Desk No. 25.0 ml. of density 0.10 M NaoH Also record desemnine volume of aceic acid" dhis calculation your Report Sheet A chemist often uses a white card with a black mark to aid in reading the meniscus of a technique make the reading more clear liquid. How does this b....
3. For the n=5 to n=2 transition: E = in nm = in Å = Color of corresponding line in the hydrogen spectrum: b. Calculate the molar concentration of the hydrochloric acid if 35.18 mL of hydrochlo- ric acid was required to neutralize 0.450 g of sodium bicarbonate to a phenolphthalein end point. C. Calculate the mass percent concentration of hydrochloric acid using the molar con- centration calculated in part band assuming the density of the solution is 1.01 g/mL....
What volume of a 0.333 M hydrobromic acid solution is required to neutralize 24.7 mL of a 0.152 M barium hydroxide solution? mL hydrobromic acid Submit Answer Retry Entire Group 6 more group attempts remaining What volume of a 0.207 M hydroiodic acid solution is required to neutralize 24.3 mL of a 0.183 M potassium hydroxide solution? mL hydroiodic acid Submit Answer Retry Entire Group 6 more group attempts remaining What volume of a 0.161 M sodium hydroxide solution is...
Please help, I'm so confused!!!! This is due wednesday night!!!
i'm gonna fail :((((
pH of Buffer Solutions Procedure: Acetic Acid-Sodium Acetate Buffer (pKa acetic acid = 4.75) Weigh about 3.5 g of Na2C2H302 3H2O, record the exact mass, and add to a 250 ml beaker. Measure exactly 8.8 mL of 3.0 M acetic acid (use 10 mL grad cylinder) and add to the beaker containing the sodium acetate. • Measure exactly 55.6 mL of distilled water and add to...
3) Assume that the pH of rain is 4.0 and that the acidity is due entirely to HNO3(a poor assumption---typically, H2SO4 is a greater contributor to acid rain than HNO3). Calculate the mass of the primary pollutant NO that was required to acidify 1 L of rain. Assume that each mole of NO is oxidized to one mole of HNO3.
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...
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...
I would like help understanding these questions.
Thank you for your time!
Acids/Bases 1. Calculate the volume (in mL) of a 1.75 M KOH solution required to completely titrate (neutralize) 16.0 mL of a 3.00 M phosphoric acid solution. 2. Calculate the concentration of a sodium hydroxide solution that required 43.40 mL to completely titrate 26.50 mL of a 0.350 M oxalic acid (H2C2O4) solution. 3. Calculate the pH of the following: (a) a solution containing a hydronium concentration of...
Due ; Went so CIVE.3620 Homework: Environmental Chemistrye hem (Note: A similar problem was previously a 20/100 point question on an hour exam.) 8. Strong bas es and strong acids completely dissociate in solution. e ttration of strong acids and bases the following neutralization reaction occurs: H OH strong base. H2O. Nitric acid and sodium hydroxide are a strong acid and a A solution cont sodium hydroxide (NaOH) th taining nitric acid (HNO,) is to be used in the neutralization...
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