Synthesis of Aspirin1

Describe the blood hydrogen carbonate buffer system. What happens when blood acidity rises? Show the equation. What happens when the blood becomes more alkaline? Show the equation. Distinguish between strong and weak acid. List some clinical uses of these acids and write equations for their dissociation in water. Did you find any of these to be a challenge? Why or why not?

The value of the solubility product constant, _____. a. Decreases with a rise in temperature b. Increases with a rise in pressure c. Is unaffected by stirring d. depends on its environment

What process is responsible for the increase in the total negative charge as soil pH increases?    a. Deprotonation   b. Protonation   c. H+ bond formation   d. Dehydration reaction

Name the two ways that remove the most carbon dioxide from the atmosphere.  Carbon dioxide combines with water to form a single product.  Name that product (label it as product #1).  That product #1 reacts with water to produce hydronium ion and product #2.  Name product #2.  BRIEFLY: How do these two reactions affect ocean pH?  BRIEFLY: how does ocean pH affect ocean-dwelling organisms?

6) Write a balanced equation for the neutralization of hydrobromic acid with potassium hydroxide.

A 1 liter solution contains 0.514 M hydrocyanic acid and 0.386 M potassium cyanide. What will the addition of 0.193 moles of hydrobromic acid do? (Assume that the volume does not change upon the addition of hydrobromic acid.) *More than one answer is accepted. A. Raise the pH slightly B. Lower the pH slightly C. Raise the pH by several units D. Lower the pH by several units E. Not change the pH F. Exceed the buffer capacity

Pls help ASAP ON ALL ASKED QUESTIONS PLS PLS

1. Copper oxides are a product of the oxidation of copper that often form on the inside of copper pipes transporting water and serves to protect the pipes against corrosion. They are toxic. At a pH above 8, these oxides are virtually insoluble in water. As the pH of the water flowing drops below 7, the solubility of these oxides increases, and the layer begins to dissolve. Based on this knowledge, and the data collected in your lab, what implications does this have on toxic metal pollutants or other pollutants in our drinking supply when the water flowing is acidic? Would this problem become better or worse if the water flowing through the pipes was hot? 2.  The chemical obtained from red cabbage that acts as a pH indicator is a pigment called anthocyanin.  Based on your results, do you think anthocyanin is a useful indicator?  Why or why not?

Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. initial type solution initial components (check all that apply) change effect of change on pH (check one) acidic pH higher H₂O A basic add KNO3 pH lower neutral pH the same acidic pH higher B H₂O, NaOH basic add HClO4 pH lower neutral pH the same acidic pH higher C H₂O basic add KOH pH lower neutral pH the same acidic pH higher H₂O, NaOH basic add NaC104 pH lower neutral pH the same

The following tabulated data is provided to answer this question and the remaining questions in the quiz. The post lab data will appear each page so that you can refer back to this data, as needed. Review the data, then answer the first question below. The equation is H2SO4 + NaOH → Na2SO4 + H20 (note, this equation is unbalanced) The last two rows are left blank because they will be filled in by your calculations. Titration Lab Trial 1 Trial 2 Trial 3 Volume of Acid Used 20.0 mL 20.2 mL 20.8 mL Molarity of Acid Used 0.05 M 0.05 M 0.05 M Initial Buret Reading 0.00 mL 0.00 mL 0.00 mL Final Buret Reading 20.7 mL 21.0 mL 21.5 mL Volume of NaOH Used Molarity of NaOH Solution What is the correct balanced equation for the neutralization reaction? Select one: O a. H2SO4 + NaOH → Na2SO4 + H2O O b. H2SO4 + 3 NaOH → Na2SO4 + 3 H2O c. H2SO4 + NaOH → Na2SO4 + 2 H20 O d. H2SO4 + 2 N2OH → N22SO4 + 2 H2O

a. slows down chemical reactions. b. speeds up chemical reactions. c. increases the pH of a solution. d. maintains a relatively constant pH. e. works by forming salts. 24. A conjugate acid-base pair a. acts as a buffer. b. can combine with H* in a solution. Remember c. can release H to combine with OH. d. describes carbonic acid (H₂CO3) and bicarbonate ions (HCO3). e. All of these are correct. 25. Solution A is a strong acid of pH 2, and solution B is an equally strong base of pH 8. Each chemical can donate or receive a single proton. If equal amounts of solutions A and B are mixed, is the result- ing solution acidic or basic? Understand 26. Carbon dioxide that accumulates in the blood can become toxic, in part because it alters the blood pH. Some of the carbon dioxide molecules react with water to form carbonic acid (CO2 + H₂O → H₂CO3). Ned can swim across the swimming pool under water. Before diving into the water, he breathes rapidly for a few seconds, and while he is under the…

Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. initial type solution initial components (check all that apply) effect of change on pH (check one) change acidic pH higher но, кон add HC10, pH lower O pH the same O pH higher O pH lower O pH the same O pH higher O pH lower O pH the same O pH higher O pH lower A basic O neutral acidic H,0 basic add HI neutral acidic H,0 basic add Nal O neutral acidic H,0, KOH add KC10, D basic neutral O pH the same B.

Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. initial type solution initial components (check all that apply) effect of change on pH (check one) change acidic pH higher A H,0 basic add Na Br pH lower neutral pH the same acidic pH higher H,0, HI B basic add KOH pH lower neutral pH the same acidic pH higher H,0 basic add Na OF pH lower neutral pH the same acidic pH higher H,0, HI D basic add KI pH lower neutral pH the same O O OO O 00 0 0 O O O0 O O00 0

1. Formulate the reaction equation for the neutralization of acetic acid with aqueous sodium hydroxide? Define the equilibrium constant.

A solution contains a mixture of Na2CO3 and NaOH. Using phenolphthalein indicator 25 mL of mixture required 19.5 mL of 0.995 M HCl for the endpoint. With methyl orange, 25 mL of solution required 25 mL of the same HCl for the endpoint. Calculate grams per liter of Na2CO3 in the mixture.   a. 23 b. 36 c. 78 d. 11

You are given 3.56 grams of unknown acid. You dissolved it in 50.0mL of DI water and titrate it with 1.00M NaOH. The end point volume of NaOH was 19.7mL. What is the molar mass of the unknown? a. 276 g/mol b. 362 g/mol c. 198 g/mol d. 72.3 g/mol e. 181 g/mol

1. Select a product from the stock shelf and transfer the liquid to a test tube. 2. Select a paper pH test strip. Record the color of the test strip in the data chart. Transfer it to the same test tube. 3. Note any color change of the paper and record in the data chart. 4. Drag the test tube containing the test strip over to the color chart to determine the pH range indicated by the paper. Record your results. 5. Record your conclusion about whether the substance is an acid, a base, or a neutral substance. 6. Repeat for all substances.

Using a pH meter, verify that 100 mL of distilled water is neutral.Dissolve 50.0 mg of naproxen drug substance, accurately weighed, in 50 mL of methanol. Add 25 mL of the neutralized water and mix. Add two drops ofphenolphthalein as the indicator. What is the blank sample in this experiment? How many sample and blank titrations are required for this experiment? Use the equation below to calculate your expected end-point volume. Each mL of 0.01 N sodium hydroxide is equivalent to 2.303 mg of naproxen,C14H14O3

When performing a titration in the lab, which equipment is not used? 1. burette 2. pipette 3. funnel 4. watch glass 5. Erlenmeyer flask