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chemistry
organic chemistry

Questions and Answers of Organic Chemistry

If the pH is 8.0 at the equivalence point for the titration of a certain weak acid with sodium hydroxide, what indicator might you use? (See Figure 15.10.) Explain your choice.Figure 15.10
a. For each of the following salts, write the reaction that occurs when it dissociates in water: NaCl(s), NaCN(s), KClO2(s), NH4NO3(s), KBr(aq), and NaF(s). b. Consider each of the reactions that you
a. When 0.10 mol of the ionic solid NaX, where X is an unknown anion, is dissolved in enough water to make 1.0 L of Concept Explorations solution, the pH of the solution is 9.12. When 0.10 mol of the
Which of the following beakers best represents a container of a weak acid, HA, in water? (Water molecules have been omitted for clarity.)
You have 0.10-mol samples of three acids identified simply as HX, HY, and HZ. For each acid, you make up 0.10 M solutions by adding sufficient water to each of the acid samples. When you measure the
What reaction occurs when each of the following is dissolved in water? a. HF b. NaF c. C6H5NH2 d. C6H5NH3Cl
You have the following solutions, all of the same molar concentration: KBr, HBr, CH3NH2, and NH4Cl. Rank them from the lowest to the highest hydroxide-ion concentration.
Rantidine is a nitrogen base that is used to control stomach acidity by suppressing the stomach's production of hydrochloric acid. The compound is present in Zantac® as the chloride salt
A chemist prepares dilute solutions of equal molar concentrations of NH3, NH4Br, NaF, and NaCl. Rank these solutions from highest pH to lowest pH.
You want to prepare a buffer solution that has a pH equal to the pKa of the acid component of the buffer. If you have 100 mL of a 0.10 M solution of the acid HA, what volume and concentration of NaA
Briefly describe two methods for determining Ka for a weak acid.
A friend of yours has performed three titrations: strong acid with a strong base, weak acid with a strong base, and weak base with a strong acid. He hands you the three titration curves, saying he
You are given the following acid€“base titration data, where each point on the graph represents the pH after adding a given volume of titrant (the substance being added during the
The three flasks shown below depict the titration of an aqueous NaOH solution with HCl at different points. One represents the titration prior to the equivalence point, another represents the
Write chemical equations for the acid ionizations of each of the following weak acids (express these in terms of H3O+). a. HBrO (hypobromous acid) b. HClO2 (chlorous acid) c. HNO2 (nitrous acid) d.
Write chemical equations for the acid ionizations of each of the following weak acids (express these in terms of H3O+). a. HCO2H (formic acid) b. HF (hydrofluoric acid) c. HN3 (hydrazoic acid) d.
Acrylic acid, whose formula is HC3H3O2 or HO2CCH=CH2, is used in the manufacture of plastics. A 0.10 M aqueous solution of acrylic acid has a pH of 2.63. What is Ka for acrylic acid?
Heavy metal azides, which are salts of hydrazoic acid, HN3, are used as explosive detonators. A solution of 0.20 M hydrazoic acid has a pH of 3.21. What is the Ka for hydrazoic acid?
Boric acid, B(OH)3, is used as a mild antiseptic. What is the pH of a 0.021 M aqueous solution of boric acid? What is the degree of ionization of boric acid in this solution? The hydronium ion arises
Formic acid, HCHO2, is used to make methyl formate (a fumigant for dried fruit) and ethyl formate (an artificial rum flavor). What is the pH of a 0.10 M solution of formic acid? What is the degree of
C6H4NH2COOH, para-aminobenzoic acid (PABA), is used in some sunscreen agents. Calculate the concentrations of hydronium ion and para-aminobenzoate ion, C6H4NH2COO, in a 0.055 M solution of the acid.
Describe how the degree of ionization of a weak acid changes as the concentration increases.
Barbituric acid, HC4H3N2O3, is used to prepare various barbiturate drugs (used as sedatives). Calculate the concentrations of hydronium ion and barbiturate ion in a 0.10 M solution of the acid. The
A solution of acetic acid, HC2H3O2, on a laboratory shelf was of undetermined concentration. If the pH of the solution was found to be 2.68, what was the concentration of the acetic acid?
A chemist wanted to determine the concentration of a solution of lactic acid, HC3H5O3. She found that the pH of the solution was 2.51. What was the concentration of the solution? The Ka of lactic
Hydrofluoric acid, HF, unlike hydrochloric acid, is a weak electrolyte. What is the hydronium-ion concentration and the pH of a 0.040 M aqueous solution of HF?
Chloroacetic acid, HC2H2ClO2, has a greater acid strength than acetic acid, because the electronegative chlorine atom pulls electrons away from the O--H bond and thus weakens it. Calculate the
What is the hydronium-ion concentration of a 2.00 M solution of 2,6-dinitrobenzoic acid, (NO2)2C6H3COOH, for which Ka = 7.94 × 10-2?
What is the hydronium-ion concentration of a 2.00 × 10-4 M solution of p-bromobenzoic acid, BrC6H4COOH, for which Ka = 1.00 × 10-4?
Phthalic acid, H2C8H4O4, is a diprotic acid used in the synthesis of phenolphthalein indicator. Ka1 = 1.2 × 10–3, and Ka2 = 3.9 × 10–6.
Carbonic acid, H2CO3, can be found in a wide variety of body fluids (from dissolved CO2).
Write the chemical equation for the base ionization of methylamine, CH3NH2. Write the Kb expression for methylamine.
Consider a solution of 0.0010 M HF (Ka = 6.8 × 10–4). In solving for the concentrations of species in this solution, could you use the simplifying assumption in which you neglect x in the
Write the chemical equation for the base ionization of aniline, C6H5NH2. Write the Kb expression for aniline.
Ethanolamine, HOC2H4NH2, is a viscous liquid with an ammonialike odor; it is used to remove hydrogen sulfide from natural gas. A 0.15 Maqueous solution of ethanolamine has a pH of 11.34. What is Kb
Trimethylamine, (CH3)3N, is a gas with a fishy, ammonialike odor. An aqueous solution that is 0.25 M trimethylamine has a pH of 11.63. What is Kb for trimethylamine?
What is the concentration of hydroxide ion in a 0.060 M aqueous solution of methylamine, CH3NH2? What is the pH?
What is the concentration of hydroxide ion in a 0.18 M aqueous solution of hydroxylamine, NH2OH? What is the pH?
Note whether hydrolysis occurs for each of the following ions. If hydrolysis does occur, write the chemical equation for it. Then write the equilibrium expression for the acid or base ionization
Note whether hydrolysis occurs for each of the following ions. If hydrolysis does occur, write the chemical equation for it. Then write the equilibrium expression for the acid or base ionization
Write the equation for the acid ionization of the Zn(H2O)62+ ion.
Write the equation for the acid ionization of the Cu(H2O)62+ ion.
For each of the following salts, indicate whether the aqueous solution will be acidic, basic, or neutral. a. Fe(NO3)3 b. Na2CO3 c. Ca(CN)2 d. NH4ClO4
Phosphorous acid, H2PHO3, is a diprotic acid. Write equations for the acid ionizations. Write the expressions for Ka1 and Ka2.
Note whether the aqueous solution of each of the following salts will be acidic, basic, or neutral.a. Na2Sb. Cu(NO3)2c. KClO4d. CH3NH3Cl
Decide whether solutions of the following salts are acidic, neutral, or basic. a. Ammonium acetate b. Anilinium acetate
Decide whether solutions of the following salts are acidic, neutral, or basic. a. Ammonium cyanate b. Anilinium cyanate
Obtain (a) The Kb value for NO2; (b) The Ka value for C5H5NH+ (pyridinium ion).
Obtain (a) The Kb value for ClO; (b) The Ka value for NH3OH+ (hydroxylammonium ion).
What is the pH of a 0.025 M aqueous solution of sodium propionate, NaC3H5O2? What is the concentration of propionic acid in the solution?
Calculate the OH concentration and pH of a 0.0020 M aqueous solution of sodium cyanide, NaCN. Finally, obtain the hydronium-ion, CN, and HCN concentrations.
Calculate the concentration of pyridine, C5H5N, in a solution that is 0.15 M pyridinium bromide, C5H5NHBr. What is the pH of the solution?
What is the pH of a 0.35 M solution of methylammonium chloride, CH3NH3Cl? What is the concentration of methylamine in the solution?
Calculate the degree of ionization of (a) 0.75 M HF (hydrofluoric acid);
What is the concentration of oxalate ion, C2O42, in 0.10 M oxalic acid, H2C2O4? Ka1 is 5.6 × 10–2, and Ka2 is 5.1 × 10–5.
Calculate the degree of ionization of (a) 0.22 M HCHO2 (formic acid);
What is the pH of a solution that is 0.10 M KNO2 and 0.15 M HNO2 (nitrous acid)?
What is the pH of a solution that is 0.20 M KOCN and 0.10 M HOCN (cyanic acid)?
What is the pH of a solution that is 0.10 M CH3NH2 (methylamine) and 0.15 M CH3NH3Cl (methylammonium chloride)?
What is the pH of a solution that is 0.15 M C2H5NH2 (ethylamine) and 0.10 M C2H5NH3Br (ethylammonium bromide)?
A buffer is prepared by adding 45.0 mL of 0.15 M NaF to 35.0 mL of 0.10 M HF. What is the pH of the final solution?
A buffer is prepared by adding 115 mL of 0.30 M NH3 to 145 mL of 0.15 MNH4NO3. What is the pH of the final solution?
What is the pH of a buffer solution that is 0.10 M NH3 and 0.10 M NH4+? What is the pH if 12 mL of 0.20 M hydrochloric acid is added to 125 mL of buffer?
A buffer is prepared by mixing 525 mL of 0.50 M formic acid, HCHO2, and 475 mL of 0.50 M sodium formate, NaCHO2. Calculate the pH. What would be the pH of 85 mL of the buffer to which 8.6 mL of 0.15
What is the pH of a buffer solution that is 0.15 M chloroacetic acid and 0.10 M sodium chloroacetate? Ka = 1.3 × 10-3.
Write the equation for the ionization of aniline, C6H5NH2, in aqueous solution. Write the expression for Kb.
What is the pH of a buffer solution that is 0.10 M propionic acid and 0.20 M sodium propionate?
What is the pH of a buffer solution that is 0.15 Mpyridine and 0.10 M pyridinium bromide?
What is the pH of a buffer solution that is 0.15 M methylamine and 0.20 M methylammonium chloride?
How many moles of sodium acetate must be added to 2.0 L of 0.10 M acetic acid to give a solution that has a pH equal to 5.00? Ignore the volume change due to the addition of sodium acetate.
How many moles of hydrofluoric acid, HF, must be added to 500.0 mL of 0.25 M sodium fluoride to give a buffer of pH 3.50? Ignore the volume change due to the addition of hydrofluoric acid.
What is the pH of a solution in which 15 mL of 0.10 M NaOH is added to 25 mL of 0.10 M HCl?
What is the pH of a solution in which 40 mL of 0.10 M NaOH is added to 25 mL of 0.10 M HCl?
A 1.24-g sample of benzoic acid was dissolved in water to give 50.0 mL of solution. This solution was titrated with 0.180 M NaOH. What was the pH of the solution when the equivalence point was
A 0.400-g sample of propionic acid was dissolved in water to give 50.0 mL of solution. This solution was titrated with 0.150 M NaOH. What was the pH of the solution when the equivalence point was
Find the pH of the solution obtained when 32 mL of 0.087 M ethylamine is titrated to the equivalence point with 0.15 M HCl.
Which of the following is the strongest base: NH3, C6H5NH2, or CH3NH2? See Table 16.2.
What is the pH at the equivalence point when 22 mL of 0.20 M hydroxylamine is titrated with 0.15 M HCl?
A 50.0-mL sample of a 0.100 M solution of NaCN is titrated by 0.200 M HCl. Kb for CN is 2.0 × 10-5. Calculate the pH of the solution: a. Prior to the start of the titration; b. After the addition
Sodium benzoate, NaC7H5O2, is used as a preservative in foods. Consider a 50.0-mL sample of 0.250 M NaC7H5O2 being titrated by 0.200 M HBr. Calculate the pH of the solution: a. When no HBr has been
Calculate the pH of a solution obtained by mixing 500.0 mL of 0.10 M NH3 with 200.0 mL of 0.15 M HCl.
Calculate the pH of a solution obtained by mixing 35.0 mL of 0.15 M acetic acid with 25.0 mL of 0.10 M sodium acetate.
Salicylic acid, C6H4OHCOOH, is used in the manufacture of acetylsalicylic acid (aspirin) and methyl salicylate (wintergreen flavor). A saturated solution of salicylic acid contains 2.2 g of the acid
Cyanoacetic acid, CH2CNCOOH, is used in the manufacture of barbiturate drugs. An aqueous solution containing 5.0 g in a liter of solution has a pH of 1.89. What is the value of Ka?
A 0.050 M aqueous solution of sodium hydrogen sulfate, NaHSO4, has a pH of 1.73. Calculate Ka2 for sulfuric acid. Sulfuric acid is a strong electrolyte, so you can ignore hydrolysis of the HSO4 ion.
A 0.10 M aqueous solution of sodium dihydrogen phosphate, NaH2PO4, has a pH of 4.10. Calculate Ka2 for phosphoric acid. You can ignore hydrolysis of the H2PO4 ion.
Calculate the base-ionization constants for CN and CO32. Which ion is the stronger base?
Give solubility product expressions for the following: a. Barium sulfate; b. Iron(III) hydroxide; c. Calcium phosphate.
Will silver iodide precipitate from a solution that is 0.0045 M AgNO3, 0.15 M NaI, and 0.20 M KCN?
What is the molar solubility of AgBr in 1.0 M Na2S2O3 (sodium thiosulfate)? Silver ion forms the complex ion Ag(S2O3)23. See Tables 17.1 and 17.2 for data.
Silver ion may be recovered from used photographic fixing solution by precipitating it as silver chloride. The solubility of silver chloride is 1.9 × 10-3 g/L. Calculate Ksp.
Lead(II) arsenate, Pb3(AsO4)2, has been used as an insecticide. It is only slightly soluble in water. If the solubility is 3.0 × 10–5 g/L, what is the solubility product constant? Assume that the
Anhydrite is a calcium sulfate mineral deposited when seawater evaporates. What is the solubility of calcium sulfate, in grams per liter? Table 17.1 gives the solubility product constant for calcium
a. Calculate the molar solubility of barium fluoride, BaF2, in water at 25°C. The solubility product constant for BaF2 at this temperature is 1.0 × 10–6. b. What is the molar solubility of barium
Anhydrite is a mineral composed of CaSO4 (calcium sulfate). An inland lake has Ca2+ and SO42 concentrations of 0.0052 M and 0.0041 M, respectively. If these concentrations were doubled by
A solution of 0.00016 M lead(II) nitrate, Pb(NO3)2, was poured into 456 mL of 0.00023 M sodium sulfate, Na2SO4. Would a precipitate of lead(II) sulfate, PbSO4, be expected to form if 255 mL of the
Which salt would have its solubility more affected by changes in pH, silver chloride or silver cyanide?
What is the concentration of Cu2+(aq) in a solution that was originally 0.015 M Cu(NO3)2 and 0.100 M NH3? The Cu2+ ion forms the complex ion Cu(NH3)42+. Its formation constant is given in Table
Lead compounds have been used as paint pigments, but because the lead(II) ion is toxic, the use of lead paints in homes is now prohibited. Which of the following lead(II) compounds would yield the
Suppose you have equal volumes of saturated solutions of NaNO3, Na2SO4, and PbS. Which solution would dissolve the most lead(II) sulfate, PbSO4?

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