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chemistry
organic chemistry

Questions and Answers of Organic Chemistry

What is the pH of a sample of gastric juice (digestive juice in the stomach) whose hydronium-ion concentration is 0.045 M?
A saturated solution of calcium hydroxide has a hydroxide-ion concentration of 0.025 M. What is the pH of the solution?
A brand of carbonated beverage has a pH of 3.16. What is the hydronium-ion concentration of the beverage?
Chemists in the seventeenth century discovered that the substance that gives red ants their irritating bite is an acid with the formula HCHO2. They called this substance formic acid after the ant,
Formic acid, HCHO2, is a stronger acid than acetic acid, HC2H3O2. Which is the stronger base, formate ion, CHO2, or acetate ion, C2H3O2?
Rank the following solutions from most acidic to most basic (water molecules have been omitted for clarity).
You have solutions of NH3, HCl, NaOH, and HC2H3O2 (acetic acid), all with the same solute concentrations. Rank these solutions in order of pH, from the highest to the lowest.
Which of the following are strong acids? Which are weak acids? (a) HC2H3O2; (b) HClO; (c) HCl; (d) HNO3; (e) HNO2; (f) HCN
What is meant by the self-ionization of water? Write the expression for Kw. What is its value at 25οC?
A 2.500-g sample of a mixture of sodium carbonate and sodium chloride is dissolved in 25.00 mL of 0.798 M HCl. Some acid remains after the treatment of the sample.a. Write the net ionic equation for
The bicarbonate ion has the ability to act as an acid in the presence of a base and as a base in the presence of an acid, so it is said to be amphiprotic. Illustrate this behavior with water by
The dihydrogen phosphate ion has the ability to act as an acid in the presence of a base and as a base in the presence of an acid. What is this property called? Illustrate this behavior with water by
The hydride ion does not exist in water because it has a greater attraction for the hydronium ion than the hydroxide ion does. Write the equation for the reaction that occurs when calcium hydride is
The nitride ion and the amide ion, NH2, have greater attractions for the hydronium ion than the hydroxide ion does. Write the equations for the reactions that occur when calcium nitride and sodium
Pure liquid hydrogen fluoride ionizes in a way similar to that of water. a. Write the equilibrium reaction for the self-ionization of liquid hydrogen fluoride. b. Will sodium fluoride be an acid or a
Pure liquid ammonia ionizes in a way similar to that of water. a. Write the equilibrium reaction of liquid ammonia. b. Will sodium amide, NaNH2, be an acid or a base in liquid ammonia? Why? c.
A solution contains 4.25 g of ammonia per 250.0 mL of solution. Electrical conductivity measurements at 25°C show that 0.42% of the ammonia has reacted with water. Write the equation for this
A solution contains 0.675 g of ethylamine, C2H5NH2, per 100.0 mL of solution. Electrical conductivity measurements at 20°C show that 0.98% of the ethylamine has reacted with water. Write the
Why do medicines frequently taste bitter?
What is meant by the pH of a solution? Describe two ways of measuring pH.
Show how methylamine, CH3NH2, is a Bronsted–Lowry base. Is methylamine also a Lewis base? Explain.
Explain how sodium hydroxide dissolves grease and hair from a stopped drain.
How is sodium hydroxide prepared commercially?
Ethanol (ethyl alcohol), CH3CH2OH, can act as a Brønsted–Lowry acid. Write the chemical equation for the reaction of ethanol as an acid with hydroxide ion, OH. Ethanol can also react as a
Ethanol, CH3CH2OH, can undergo self-ionization. Write the chemical equation for this self-ionization. Explain how you arrived at this equation. At room temperature, the ion product for this
Aluminum chloride, AlCl3, reacts with trimethylamine, N(CH3)3. What would you guess to be the product of this reaction? Explain why you think so. Describe the reaction in terms of one of the
Consider each of the following pairs of compounds, and indicate which one of each pair is the stronger Lewis acid. Explain how you arrived at your answers.a. Fe2+, Fe3+b. BF3, BCl3
Arrange each of the following in order of increasing acidity. You may need to use a couple of rules to decide the order for a given series. Explain the reasoning you use in each case.a. HBrO2, HBrO3,
The following is a table of some of the oxoacids of the halogens. Which acid in the table is the strongest? Which is the weakest? Explain how you arrived at your answers.
Suppose you have 557 mL of 0.0300 MHCl, and you want to make up a solution of HCl that has a pH of 1.831. What is the maximum volume (in liters) that you can make of this solution?
How many grams of water are in dissociated form (as H+ and OH ions) in 1.00 L of pure water? How many hydrogen ions, H+(aq), are there in 1.00 L of pure water?
You want to make up 3.00 L of aqueous hydrochloric acid, HCl(aq), that has a pH of 2.00. How many grams of concentrated hydrochloric acid will you need? Concentrated hydrochloric acid contains 37.2
You can obtain the pH of a 0.100 M HCl solution by assuming that all of the H3O+ ion comes from the HCl, in which case the pH equals log 0.100 = 1.00. But if you want the pH of a solution that is
Phosphorous acid, H3PO3, and phosphoric acid, H3PO4, have approximately the same acid strengths. From this information, and noting the possibility that one or more hydrogen atoms may be directly
Hypophosphorous acid, H3PO2, and phosphoric acid, H3PO4, have approximately the same acid strengths. From this information, and noting the possibility that one or more hydrogen atoms may be directly
Boron trifluoride, BF3, and ammonia, NH3, react to produce BF3NH3. A coordinate covalent bond is formed between the boron atom on BF3 and the nitrogen atom on NH3. Write the equation for this
Boron trifluoride, BF3, and diethyl ether, (C2H5)2O, react to produce a compound with the formula BF3 ∙ (C2H5)2O. A coordinate covalent bond is formed between the boron atom on BF3 and the oxygen
What is the pH of a neutral solution at 37οC, where Kw equals 2.5 × 10-14?
You make a solution by dissolving 0.0010 mol of HCl in enough water to make 1.0 L of solution.a. Write the chemical equation for the reaction of HCl(aq) and water.b. Without performing calculations,
Describe any thermochemical (heat of reaction) evidence for the Arrhenius concept.
Two 0.10-mol samples of the hypothetical monoprotic acids HA(aq) and HB(aq) are used to prepare 1.0-L stock solutions of each acid.a. Write the chemical reactions for these acids in water. What are
Aqueous solutions of ammonia, NH3, were once thought to be solutions of an ionic compound (ammonium hydroxide, NH4OH) in order to explain how the solutions could contain hydroxide ion. Using the
Blood contains several substances that minimize changes in its acidity by reacting with either an acid or a base. One of these is the hydrogen phosphate ion, HPO42. Write one equation showing this
Compare the structures of HNO2 and H2CO3. Which would you expect to be the stronger acid? Explain your choice.
The value of the ion-product constant for water, Kw, increases with temperature. What will be the effect of lowering the temperature on the pH of pure water?
You make solutions of ammonia and sodium hydroxide by adding the same moles of each solute to equal volumes of water. Which solution would you expect to have the higher pH?
A strong monoprotic acid, with the molecular structure, is dissolved in a beaker of water. Which of the following pictures best represents the acid solution (water molecules have been omitted for
A weak acid, HA, is dissolved in water. Which one of the following beakers represents the resulting solution? (Water molecules have been omitted for clarity.)
Write the balanced reaction of hydroxide ion with hydrofluoric acid, HF, to form fluoride ion and water. Identify each species as either an acid or a base.
Define an acid and a base according to the Brønsted–Lowry concept. Give an acid–base equation and identify each species as an acid or a base.
Write the balanced reaction of hypochlorous acid, HOCl, with water to form hydronium ion and the conjugate base of HOCl. Identify each species as either an acid or a base.
Give the conjugate base to each of the following species regarded as acids. a. HPO42 b. H2S c. HNO2 d. H2AsO4
Give the conjugate base to each of the following species regarded as acids. a. HSeO4 b. PH4+ c. HS d. HOCl
Give the conjugate acid to each of the following species regarded as bases. a. ClO b. AsH3 c. H2PO4 d. TeO32
Give the conjugate acid to each of the following species regarded as bases. a. HSe b. NH2 c. ClO2 d. N2H4
For the following reactions, label each species as an acid or a base. Indicate the species that are conjugates of one another.a.b. c. d.
For the following reactions, label each species as an acid or a base. Indicate the species that are conjugates of one another.a.b. c. d.
The following shows ball-and-stick models of the reactants in a Lewis acid€“base reaction.Write the complete equation for the reaction, including the product. Identify each reactant as a
The following shows ball-and-stick models of the reactants in a Lewis acid€“base reaction.Write the complete equation for the reaction, including the product. Identify each reactant as a
Complete each of the following equations. Then write the Lewis formulas of the reactants and products and identify each reactant as a Lewis acid or a Lewis base. a. AlCl3 + Cl → b. I + I2 →
What is meant by the conjugate acid of a base?
Complete each of the following equations. Then write the Lewis formulas of the reactants and products and identify each reactant as a Lewis acid or a Lewis base. a. GaBr3 + Br → b. BF3 + F→
In the following reactions, identify each reactant as a Lewis acid or a Lewis base. a. Cu2+ + 6H2O → Cu(H2O)62+ b. BBr3 + :AsH3 → Br3B:AsH3
In the following reactions, label each reactant as a Lewis acid or a Lewis base. a. BeF2 + 2F → BeF42 b. SnCl4 + 2Cl → SnCl62
Natural gas frequently contains hydrogen sulfide, H2S. H2S is removed from natural gas by passing it through aqueous ethanolamine, HOCH2CH2NH2 (an ammonia derivative), which reacts with the hydrogen
Coal and other fossil fuels usually contain sulfur compounds that produce sulfur dioxide, SO2, when burned. One possible way to remove the sulfur dioxide is to pass the combustion gases into a tower
Complete the following equation. Using Table 15.2, predict whether you would expect the reaction to occur to any significant extent or whether the reaction is more likely to occur in the opposite
Complete the following equation. Using Table 15.2, predict whether you would expect the reaction to occur to any significant extent or whether the reaction is more likely to occur in the opposite
Use Table 15.2 to decide whether the species on the left or those on the right are favored by the reaction.a.b. c. d.
Use Table 15.2 to decide whether the species on the left or those on the right are favored by the reaction.a.b. c. d.
Write an equation in which H2PO3 acts as an acid and another in which it acts as a base.
For each of the following pairs, give the stronger acid. Explain your answer. a. H2S, HS b. H2SO3, H2SeO3 c. HBr, H2Se d. HIO4, HIO3 e. H2S, H2O
Order each of the following pairs by acid strength, giving the weaker acid first. Explain your answer. a. HBrO4, HBrO3 b. HCO3, H2CO3 c. H2S, H2Te d. HBr, H2Se e. H3PO4, H3AsO4
What are the concentrations of H3O+ and OH in each of the following? a. 1.2 M HBr b. 0.32 M KOH c. 0.085 M Ca(OH)2 d. 0.38 M HNO3
What are the concentrations of H3O+ and OH in each of the following? a. 1.65 M NaOH b. 0.35 M Sr(OH)2 c. 0.045 M HClO4 d. 0.58 M HCl
What are the hydronium-ion and the hydroxide-ion concentrations of a solution at 25οC that is 0.0085 M barium hydroxide, Ba(OH)2?
A saturated solution of magnesium hydroxide is 3.2 × 10-4 M Mg(OH)2. What are the hydronium-ion and hydroxide-ion concentrations in the solution at 25οC?
The following are solution concentrations. Indicate whether each solution is acidic, basic, or neutral. a. 5 × 106 M H3O+ b. 5 × 109 M OH c. 1 × 107 M OH d. 2 × 109 M H3O+
Describe four ways in which the Brønsted–Lowry concept enlarges on the Arrhenius concept.
The following are solution concentrations. Indicate whether each solution is acidic, basic, or neutral. a. 2 × 10-11 M OH b. 2 × 10-9 M H3O+ c. 6 × 10-5 M OH d. 6 × 10-3 M H3O+
A shampoo solution at 25οC has a hydroxide-ion concentration of 1.5 × 10-9 M. Is the solution acidic, neutral, or basic?
An antiseptic solution at 25οC has a hydroxide-ion concentration of 8.4 × 10-5 M. Is the solution acidic, neutral, or basic?
Which of the following pH values indicate an acidic solution at 25οC? Which are basic and which are neutral? a. 4.6 b. 7.0 c. 1.6 d. 10.5
Which of the following pH values indicate an acidic solution at 25οC? Which are basic and which are neutral? a. 5.6 b. 2.5 c. 13.2 d. 9.3
For each of the following, state whether the solution at 25°C is acidic, neutral, or basic: (a) A beverage solution has a pH of 3.5. (b) A 0.50 M solution of potassium bromide, KBr, has a pH of
For each of the following, state whether the solution at 25°C is acidic, neutral, or basic: (a) A 0.1 M solution of trisodium phosphate, Na3PO4, has a pH of 12.0. (b) A 0.1 M solution of calcium
Obtain the pH corresponding to the following hydronium-ion concentrations. a. 1.0 × 10–8 M b. 5.0 × 10–12 M c. 7.5 × 10–3 M d. 6.35 × 10–9 M
Obtain the pH corresponding to the following hydronium-ion concentrations. a. 2.5 × 10-4 M b. 5.7 × 10-10 M c. 4.6 × 10-5 M d. 2.91 × 10-11 M
A sample of vinegar has a hydronium-ion concentration of 7.5 × 10–3 M. What is the pH of the vinegar?
Define an acid and a base according to the Lewis concept. Give a chemical equation to illustrate.
Some lemon juice has a hydronium-ion concentration of 5.0 × 10-3 M. What is the pH of the lemon juice?
Obtain the pH corresponding to the following hydroxide-ion concentrations.a. 5.25 × 10–9 Mb. 8.3 × 10–3 Mc. 3.6 × 10–12 Md. 2.1 × 10–8 M
Obtain the pH corresponding to the following hydroxide-ion concentrations.a. 6.74 × 10–11 Mb. 5.8 × 10–5 Mc. 3.4 × 10–10 Md. 7.1 × 10–4 M
A solution of washing soda (sodium carbonate, Na2CO3) has a hydroxide-ion concentration of 0.0040 M. What is the pH at 25°C?
A solution of lye (sodium hydroxide, NaOH) has a hydroxide-ion concentration of 0.050 M. What is the pH at 25°C?
The pH of a cup of coffee (at 25°C) was found to be 5.12. What is the hydronium-ion concentration?
A wine was tested for acidity, and its pH was found to be 3.85 at 25°C. What is the hydronium-ion concentration?
A detergent solution has a pH of 11.63 at 25°C. What is the hydroxide-ion concentration?
Morphine is a narcotic that is used to relieve pain. A solution of morphine has a pH of 9.61 at 25°C. What is the hydroxide-ion concentration?
A 1.00-L aqueous solution contained 5.80 g of sodium hydroxide, NaOH. What was the pH of the solution at 25°C?

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