Lesson 2-Minor Comp-23

The metabolic disorder diabetes causes a buildup of acetone CH3COCH3 in the blood. Acetone a volatile compound is exhaled giving the breath of intreated diabetes a distinctive odor. The acetone is produced by a breakdown of fats in a series of reactions. The equation for the last step the breakdown of acetoacetic acid to give acetone and CO2 is CH3COCH2CO2H->CH3COCH3+CO2. What mass of acetone can be produced from 125 mg of acetoacetic acid?

We want to determine the acetylsalicyclic acid content of a series of aspirin tablets by titration with NaOH(aq). Each of the tablets is expected to contain about 0.32 g of HC9H7O4. What molarity of NaOH(aq) should we use for titration volumes of about 23 mL? HC9H7O4(aq) + OH-(aq)  C9H7O4-(aq) + H2O(l)

An unkown solid acid is either citric acid or tartaric acid. To determine which acid you have, you titrate a sample of the solid with NaOH. The appropriate reactions are as follows: Citric acid: H3C6H5O7 (aq) + 3 NaOH (aq) --> 3 H2O (l) + Na3C6H5O7 (aq)   Tartaric acid: H2C4H4O6 (aq) + 2 NaOH (aq) --> 2 H2O (l) + Na2C4H4O6 (aq)   A 0.956 g sample requires 29.1 ml of 0.513 M NaOH for titration to the equivalence point. What is the unknown acid?

A sample of hydrochloric acid is standardized using sodium bicarbonate, NaHCO3. A.) Write the balanced chemical equation for the reaction of hydrochloric acid with sodium bicarbonate. B.) Calculate the molar concentration of the hydrochloric acid if 35.18 mL of hydrochloric 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 concentration calculated in part b and assuming the density of the solution is 1.01 g/mL.

When butanoic acid (C3H7COOH) reacts with the strong base potassium hydroxide (KOH), potassium butanoate (C3H7COOK), a salt of the weak acid is formed. Write a balanced chemical equation with physical states to show the dissociation of the potassium butanoate (C3H7COOK).

Give the correct chemical formulas of the products of an acid-base neutralization between H2SO4 and Al(OH)3.  (Numbers will be assumed to be subscripts in your answer.)  Do not try to enter any physical states or coefficients in the answer boxes.  The order in which you list the products does not matter. Formula of one product (do not include the coefficient):  Answer      Formula of other product (do not include the coefficient):  Answer What is the biggest coefficient in the balanced chemical equation for the reaction?  (Report a single digit for your answer.)  Answer

true or false?  The following reaction equation is a redox reaction: 2H2O (l) + 2Cl- (aq) ⟶ H2 (g) + Cl2 (g) + 2OH- (aq)

I have 3.025 lb H2SO4 and 200 gal of water.  How many molecules of sulfuric acid do I have?  What is the pH? All hydrogen atoms convert to hydronium ions. 1 oz= 28.35 g 1 gall=3.785 L

Give the correct chemical formulas of the products of an acid-base neutralization between H2SO4 and KOH.  (Numbers will be assumed to be subscripts in your answer.)  Do not try to enter any physical states or coefficients in the answer boxes.  The order in which you list the products does not matter.   What is the coefficient in front of the KOH in the balanced equation for the reaction?  (Report a single digit for your answer.)

The balanced molecular equation for complete neutralization of H 2SO 4 by KOH in aqueous solution is H2SO4 (aq) + 2КОН (аq) — 2H20 (I) + К2S04 (s) B H2SO4 (aq) + 20H- (aq) → 2H2O (I) + SO42- (aq) (C) 2H+ (aq) + 20H- (aq) → 2H2O (I) D H2SO4 (aq) + 2KOH (aq) – 2H2O (I) + K2SO4 (aq) 2H+ (aq) + 2KOH (aq) → 2H2O (I) + 2K+ (aq) E.

Give Detailed Solution (don't give Handwritten answer

NaHCO3 (aq) + CH3 COOH (aq) —> CO2 (g) + H2O (l) + CH3 COONa (aq)   Calculate the molar concentration of 100ml of vinegar (CH3COOH) and 2.5 ml of baking soda (NaHCO3). Note that the concentration of table vinegar is about 1 mol/L and the density of baking soda is 2.2 g/cm3

what is the mass of AgNO3 that is represent in "solution 3"(please use three significant figures for the answer)

7. A student weighs out exactly 1.562 grams of p-aminophenol and exactly 40 mL of water. After dissolving p-aminophenol in HCI, 10 mL of acetic anhydride is added. The student follows the procedure and acetaminophen is prepared. What is the maximum amount of acetaminophen she could obtain from the reaction if the percentage yield is 76%? I

A student is given an antacid tablet that weighs 5.9200 g. The tablet is crushed and 4.8270 g of the antacid is added to 200. mL of simulated stomach acid. It is allowed to react and then filtered. It is found that 25.00 mL of this partially neutralized stomach acid required 11.7 mL of a NaOH solution to titrate it to a methyl red end point. It takes 27.8 mL of this NaOH solution to neutralize 25.00 mL of the original stomach acid. How much of the stomach acid (in mL) is neutralized by the 4.8270 g crushed sample of the tablet?

Complete the balanced chemical equation for the following reaction between a weak acid and a strong base. H₂S (aq) + KOH(aq) → 2- 3C₂² 1 2 + (s) S 3 K Reset 4 (1) 5 6 LO O 7 (g) ㅈ H 8 9 11 (aq) Submit X 0 • x H₂O

Sodium hydrogen carbonate NaHCO3, also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl, which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl(aq)+NaHCO3(aq)→NaCl(aq)+H2O(l)+CO2(g)  The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a woman suffering from indigestion can be considered to be 200.mL of a 0.089M HCl solution. What mass of NaHCO3 would she need to ingest to neutralize this much HCl? Be sure your answer has the correct number of significant digits.

Sodium hydrogen carbonate NaHCO3, also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl, which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl(aq) +NaHCO3(aq) →NaCl(aq) +H2O(l) +CO2(g) The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a woman suffering from indigestion can be considered to be 250.mL of a 0.060 M HCl solution. What mass of NaHCO3 would she need to ingest to neutralize this much HCl ?  Be sure your answer has the correct number of significant digits.

Sodium hydrogen carbonate NaHCO3, also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl, which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction:   HCl(aq)+NaHCO3(aq)→NaCl(aq)+H2O(l)+CO2(g)    The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a woman suffering from indigestion can be considered to be 250.mL of a 0.075M HCl solution. What mass of NaHCO3 would she need to ingest to neutralize this muchHCl? Be sure your answer has the correct number of significant digits.

In the aspirin preparation, 0.2 mole from salicylic, 0.8 moles from acetic anhydride, and 0.3 mole H2SO4 were used to start the reaction. Write the reaction chemical equation and calculate the efficiency of the reaction and the amount of the aspirin, if the amount of the acetic acid was 6.0g.

Sodium hydrogen carbonate (NaHCO3), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HCI), which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCI through this reaction: HCl(aq) + NaHCO3(aq) NaCl(aq) + H₂O(l) + CO₂(9) The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 200. mL of a 0.027 M HCl solution. What mass of NaHCO3 would he need to ingest to neutralize this much HCI ? Round your answer to 2 significant digits. X 5