Q: Phenylacetic acid (C6H5CH2COOH, simplified here as HPAc) builds up in the blood of persons with…
A: Answer: Given data: pH=2.62α=0.02C=0.12M
Q: Would an aqueous solution of the following salt be acidic, basic, or neutral in terms of pH?…
A: Acid is a substance that donated proton in water. Base is a substance that donates OH- in water.…
Q: Determine the Ka of a 0.10-M solution of hydrogen sulfate ion, HSO₄⁻, that is 1% ionized.
A: Ionisation of Hydrogen sulfate.
Q: The Ka, for propionic acid, HC3H5O2, is 1.30 x 10^ -5. What is the pH of a 0.0850 M propionic acid…
A: The dissociation reaction of propanoic acid is given by HC3H5O2 -----> H+ + C3H5O2- hence Ka = […
Q: In the laboratory, a general chemistry student measured the pH of a 0.453 M aqueous solution of…
A: The dissociation of acetic acid is given as, CH3COOH↔CH3COO- + H+ By definition, the acid…
Q: The hydronium ion concentration of an aqueous solution of 0.558 M acetic acid (K, = 1.80x10) is M.…
A:
Q: NH3 is a weak base (?b=1.8×10^−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…
A: Given: Kb = 1.8 × 10-5 Concentration of solution = 0.056 M Temperature = 25…
Q: The pH of a 0.0833 M ethanoic acid (Ka=1.8x10-5) solution is
A:
Q: HCN is a weak acid (Ka=6.20×10−10), so the salt, KCN , acts as a weak base. What is the pH of a…
A: Ka = 6.20×10-10 pKa = -log(Ka) = -log(6.2×10-10 = 9.21 Concentration(C) of salt =0.0750 M
Q: NH3 is a weak base (Kb=1.8×10−5 M), so the salt NH4Cl acts as a weak acid. What is the pH of a…
A: The ionization of NH4Cl as follows,
Q: A tablet containing 500 mg of aspirin was dissolved in enough water to make 100 mL of solution.…
A: Given, Mass of aspirin, C9H8O4 = 500 mg = 0.500 g (1 mg = 0.001 g) Volume of solution = 100 mL =…
Q: The pH of a 0.45 M solution of a weak acid, HA, is 2.13. What is the value of Ka for the weak acid?
A: Given data,pH=2.13Molarity of HA=0.45
Q: A 0.185 M solution of a weak acid (HA) has a pH of 2.95. Calculate the acid ionization constant (Ka)…
A: Given:
Q: If a buffer solution is 0.300 M in a weak acid -5, (K = 2.6 x 10) and 0.470 M in its conjugate base,…
A: The Henderson-Hasselbalch equation is given as,
Q: If the Ka of a monoprotic weak acid is 5.8 x 10-6, what is the pH of a 0.12 M solution of this acid?
A: Negative logarithm of Concentration of [H+] ion present in the solution is known as pH of the…
Q: What is the pH of a 2.50 molar solution of NaCN(aq)? The KA for HCN = 6.2 × 10^ -10
A: Since the NaCN salt is completely soluble in water Hence we can say concentration of NaCN =…
Q: The pH of a (1.7300x10^-1) molar solution of an aqueous weak acid (HA) is (1.99x10^0). The Ka for…
A: PHis defined as the power of Hydrogen.it measure acidity, basicity or neutrality of aqueous…
Q: The acid-dissociation constant (Ka) of hydrocyanic acid (HCN) at 25.0°C is 4.9 × 10-10. What is the…
A: NaCN → Na+ + CN- CN- + H2O ⇔ HCN + H3O+ The data given are- Ka of…
Q: calculate the pH of the equivalence pount concentraton of N2OH solution = oil mollL Mean tire (NoOH…
A: Aspirin is a weak acid. It is reacting with a strong base NaOH. So, the equivalence point will be…
Q: The pH of a 0.6 M aqueous solution of formic acid, HCHO2, at 25.0 °C is 1.7. What is the value of Ka…
A: Given that, pH of formic acid = 1.7 Concentration of formic acid = 0.6M
Q: What is the pH of a 0.380 M solution of NACN (Ka of HCN is 4.9 x 1010)?
A:
Q: Calculate the pH of a 0.50 M solution of sodium cyanide (NaCN). The K, of HCN is 4.9 x 10 10.
A: A strong base and weak acid react to form salt and water. The salt will be basic in nature and the…
Q: The value of K, for phenol (a weak acid) is 1.00×10-10. What is the value of Kp, for its conjugate…
A:
Q: What is the pH of a solution containing 6.65 g sodium acetate (NaC2H302, 82.03 g/mol) in 100.0 mL of…
A:
Q: NH3 is a weak base (Kb=1.8×10−5Kb=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the…
A:
Q: The substance benzoic acid (C6H5COOH) is a weak acid (K₂ = 6.3x10-5). What is the pH of a 0.230 M…
A:
Q: In the laboratory, a general chemistry student measured the pH of a 0.544M aqueous solution of…
A: Given :- Initial concentration of aqueous solution of acetic acid = 0.544 M pH of solution = 2.488…
Q: 500
A: Dear student I have given answer to your question in the image format.
Q: HCN is a weak acid (Ka=6.20×10−10) , so the salt, KCN , acts as a weak base. What is the pH of a…
A: Weak acid are those acid which does not dissociate completely in aqueous solution and weak base are…
Q: What is the pH of a solution that is 0.34 M KOCN and 0.14 M HOCN (cyanic acid)?
A:
Q: The Ka of a weak monoprotic acid is 1.85 x 10-5. What is the pH of a 0.0761 M solution of this acid?
A: First, we have calculated the concentration of [H+] with the help of Ka and the concentration of the…
Q: A 0.015M solution of cyanic acid has a pH of 2.67. Calculate the ionization constant, Ka, of the…
A: Given: Concentration of Cyanic acid(HCN) solution = 0.015 M pH = 2.67
Q: Calculate the pH of a 0.05 M solution of hydrofluoric acid. The Ka of hydrofluoric acid is 6.6x10^-4
A: Given data, Molarity of HF=0.05MKa of HF=6.6×10-4 pH of a solution is given by -log[H+]
Q: The pH of a 0.5 M aqueous solution of formic acid, HCHO2, at 25.0 °C is 2.0. What is the value of Ka…
A: pH tells us about the acidic or alkaline values of a solution. Dissociation of a weak acid depends…
Q: The Ka for niacin is 1.5 x 10-5. Whatis the pH of a 0.010 M solution of niacin?
A: The dissociation reaction of niacin is as shown below Hence we can see that 1 molar concentration…
Q: If the Ka of a monoprotic weak acid is 6.6x10-6, what is the pH of a 0.32 M solution of this acid?
A: Ka = 6.6 x 10-6 c = 0.32 M
Q: The Ka for cyanic acid HOCN is 3.5 x 10-4. What is the pH of a 0.37 M solution of the acid? What is…
A:
Q: A 0.785M solution of the weak acid, hypoiodous acid, HOI, has a Ka of 2.32x10-11. What is the…
A:
Q: The hydroxide ion concentration of an aqueous solution of 0.325 M phenol (a weak acid) , C6H5OH, is…
A:
Q: A 0.861 M solution of a weak base has a pH of 11.80. What is the base hydrolysis constant, K, for…
A: Hydrolysis constant Kb can be calculated by the following way .
Q: The pH of a 0.55 M aqueous solution of hypobromous acid, HBrO, at 25oC is 4.48. What is the value of…
A: The concentration of HBrO solution = 0.55 M. pH of aqueous HBrO solution = 4.48.
Q: 5 g of cyanoacetic acid, CH2CNCOOH in a liter of aqueous solution has a pH of 1.89. what is the…
A: SOLUTION Acid Dissociation Constant It is an equilibrium constant of a weak acid which…
Q: Ascorbic acid, H2C6H6O6, is a diprotic acid with Ka1 = 7.9 * 10-5 and Ka2 = 1.6 * 10-12. What is…
A: Dissociation constants of ascorbic acid given are as follows: Ascorbic Acid dissociates as…
Q: Determine the pH of a solution of a weak acid (HA) that is 0.0072 M. The Ka of the weak acid is 1.9…
A: Given , Weak acid is HA Concentration of weak acid (C) = 0.0072 M Dissociation constant (Ka) of the…
Q: The Ka of a weak monoprotic acid is 1.13 x 10-5. What is the pH of a 0.0777 M solution of this acid?…
A:
Q: Calculate the pH of a 27 mg/L solution of hydrocyanic acid (HCN). The pKa of hydrocyanic acid is…
A: Given: The concentration of hydrocyanic acid is 27 mg/L. The pKa of hydrocyanic acid is 9.3.
Q: at 25 degrees celcous, the Ka of HCO2H is 1.77 x 10^-4. What is the Delta G naught in kj/mol for…
A: Given : Ka of HCO2H = 1.77 X 10-4 And temperature = 25 oC
Q: The hydroxide ion concentration of an aqueous solution of 0.429 N acetylsalicylic acid (aspirin),…
A:
Q: Lithium dihydrogen borate (LIH2BO3) is the lithium salt of the conjugate base of boric acid. The Ka…
A: Given that - Ka for Boric acid, H3BO3 = 5.8×10-10 Then, from following formula - Ka . Kb = Kw =…
Q: What is the pH of a 1.00 molar solution of NaCN(aq)? The Ka for HCN = 6.2 × 10–10 .
A: Given information: Concentration of NaCN solution = 1.00 m The pH of a 1.00 molar solution of NaCN…
calcualate the pH of a 0.15 M solution of pyruvic acid ka of pyruvic acid is 4.1x10^-3
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- Write the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ionTable 13-4 lists the stepwise Ka values for some polyprotic acids. What is the difference between a monoprotic acid, a diprotic acid, and a triprotic acid? Most polyprotic acids are weak acids; the major exception is H2SO4. To solve for the pH of a solution of H2SO4, you must generally solve a strong acid problem as well as a weak acid problem. Explain. Write out the reactions that refer to Ka1 and Ka2 for H2SO4. For H3PO4, Ka1 = 7.5 103, Ka2 = 6.2 108, and Ka3= 4.8 1013. Write out the reactions that refer to the Ka1, Ka2and Ka3equilibrium constants. What are the three acids in a solution of H3PO4? Which acid is strongest? What are the three conjugate bases in a solution of H3PO4? Which conjugate base is strongest? Summarize the strategy for calculating the pH of a polyprotic acid in water.What is the freezing point of vinegar, which is an aqueous solution of 5.00% acetic acid, HC2H3O2, by mass (d=1.006g/cm3)?
- Which of the diagrams in Problem 10-135 represents the substance that is the weakest electrolyte?For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)Estimate the pH that results when the following two solutions are mixed. a) 50 mL of 0.3 M CH3COOH and 50 mL of 0.4 M KOH b) 100 mL of 0.3 M CH3COOH and 50 mL of 0.4 M NaOH c) 150 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2 d) 200 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2
- The pH of a 0.10-M solution of propanoic acid, CH3CH2COOH, a weak organic acid, is measured at equilibrium and found to be 2.93 at 25 °C. Calculate the Ka of propanoic acid.Acrylic acid is used in the polymer industry in the production of acrylates. Its K, is 5.6 X 10“’. What is the pH of a 0.11 M solution of acrylic acid, CH2CHCOOH?Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?
- The ionization constant of lactic acid, CH3CH(OH)CO2H, an acid found in the blood after strenuous exercise, is 1.36104. If 20.0 g of lactic acid is used to make a solution with a volume of 1.00 L, what is the concentration of hydronium ion in the solution?Consider citric acid, H3C6H5O7, added to many soft drinks. The equilibrium constants for its step-wise ionization areKa1=7.5104 ,Ka2=1.7105, andKa3=4.0107. Write the overall net ionic equation and calculate K for the complete ionization of citric acid.Two strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?