Given the ka values of the following monoprotic acids: hypochlorous acid (HClO, ka = 3.3´10-8), C6H5CO2H (ka = 6.3´10-5), HNO2 (ka = 4.5´10-4), and CH3CO2H (ka = 1.8´10-5), which of the following aqueous salt solutions is the most basic?

Q: Phosphoric acid, H3PO4 is a triprotic acid.    pKa1= 2.16      pKa2=7.21            pKa3=12.32…

A: Given data, Molarity of HPO42-=0.450MpKa1=2.16pKa2=7.21pKa3=12.32

Q: antiseptic and disinfectant in topical pharmaceutical products in the treatment of skin disorders…

A: We know that the maximum amount of solute that can be dissolved in a solvent at a particular…

Q: 2) A 0.10 M solution of which of the following salts would be predicted to exhibit a pH of 7.46 at…

A: Henderson Hasselbalch equation The equation that is used to calculate the pH of a buffer system is…

Q: Calculate the [H3O+] of a 0.280 M acid solution; Ka=3.10 x 10-9 Group of answer choices   5.92 x…

A: Given, Concentration of acid solution (C) = 0.280 M Ka value of acid = 3.10 × 10-9 [H3O+] = ? Note:…

Q: Which of the following acids would be the weakest?     HClO (Ka = 3.0 × 10-8) HNO2 (Ka = 4.5 ×…

A: We have to predict the weakest acid.

Q: A 0.25 M solution of a weak acid has an α = 3.0 %.  Calculate [H3O+] of the solution.

A: % dissosciation = 3.0 %Molarity of undissosciated acid = 0.25 MH3O+ = To be determined

Q: Place the following fictitious monoprotic acids in order of increasing acidity. HA 5 (pk a =…

A: Stronger acid has high acid dissociation constant (Ka) value.

Q: Consider the following chemical reaction and that H2SO4 is a strong acid: H2SO4 + H2O ==== HSO4- +…

A:

Q: What is the pH of a solution that is 0.10 M HNO2 and 0.10 M NaNO2 (the conjugate base)? Ka of HNO2 =…

A: To solve the pH of the solution, you can use the Henderson-Hasselbalch equation, which…

Q: the solution acidic or basic? How did you know?

A:

Q: What is the pH of a solution of 0.5 M K2CO3 and 0.45 M NaHCO3? pKa of HCO3- = 10.25. Enter your…

A:

Q: write the basic equilibrium equation that

A: Given : C3H5O2- is a base To find: Basic equilibrium equation that exists in solution.

Q: Which compound below is the stronger acid in aqueous solution? W 5.0M H2SO3 or 0.020M H2SO4…

A: To find: Which is stronger acid in solution, 5.0 M H2SO3 or 0.020 M H2SO4?

Q: Phenylethylamine is linked to the "feel-good" effect of eating chocolate. The pKb of…

A: The aim is to determine the relative strengths of phenylethylamine (P) and its conjugate acid (PH+)…

Q: 1. (a) calculate the hydrogen ion concentration in a 0.200 M solution of propanoic acid. The acid…

A: Degree of dissociation of a weak acid in a solution (α) = (Ka/C)1/2 [H+] = (Ka x C)1/2 % Ionization…

Q: Arsenic acid (H3AsO4) is a triprotic acid with K a1 = 5 X 10 -3, Ka2 = 8 X 10 -8, and Ka3 = 6 X…

A: Triprotic acid can gives 3 H+ ions at each dissociation with 3 dissociation constants. Concentration…

Q: does KOH(aq)+HCl(aq)--->KCl(aq)+H2O(l) represent an acid-base neutralization reaction? yes or no…

A: Neutralization reaction: The hydrogen ion of acid reacts with the hydroxide ion of a base to form…

Q: 2) What is the concentration of [H3O+] in a solution with [OH-] = 1 × 10-12 M? Is the solution…

A: As you have posted multiple questions, we will solve only first one as per our guideline. Please…

Q: Use hard-soft acid-base theory to predict the preferred direction for the equilibrium in each of the…

A:

Q: Propanoic acid HC3H5O2, has a Ka of 1.3 x 10-5. What is the [H3O+] in a (1.51 x 10-1) M solution of…

A: The ionization of Propanoic acid HC3H5O2 takes place as,                             HC3H5O2 (aq)  +…

Q: group of students are trying to determine whether a base is an Arrhenius base or a Bronsted-Lowry…

A: An Arrhenius acid is a substance which can donate protons while an Arrhenius base can donate…

Q: The pH of a 0.0833 M ethanoic acid (Ka=1.8x10-5) solution is

A:

Q: Arsenic acid (H3AsO4) is a triprotic acid with Ka1=5.5×10-3, Ka2 = 1.7 ×10-7, and Ka3 =5.1×10-12.…

A: Triprotic acid can gives 3 H+ ions at each dissociation with 3 dissociation constants. Concentration…

Q: The K₂ for a base is 15.3 x 10-13. What is the Ka for its conjugate acid?

A: Given :- kb for a base = 15.3 × 10-13  To determine :- value of Ka for its conjugate acid

Q: Give the products from the following acid-base reactions and identify the acid and base on the left…

A:

Q: H3PO4 is a weak acid that dissociates into H2PO4- and H+. What is the Ph of a .5 M solution of…

A:

Q: iven that acetic acid has Ka = 1.8 x 10–5, what is the pH of a solution that contains the molar…

A:

Q: The weak acid HQ has a pKₐ of 4.89.(a) Calculate the [H3O⁺] of 3.5X10⁻² M HQ.(b) Calculate the…

A: Calculation of dissociation constant:

Q: What is percent ionization of 0.0065 M chloroacetic acid? K₁ = 1.36 × 10-3 The value of Kw at the…

A:

Q: The chemical formulae of some acids are listed in the first column of the table below, and in the…

A: Since, H3PO4 is a triprotic acid it dissociates with water a follows-

Q: Calculate the pH of a 0.0712 M aqueous solution of piperidine (C5H₁1N, Kµ = 1.3×10-³). pH =

A: pH can be defined as the negative logarithm of hydrogen ion concentration. It can be given as…

Q: Arsenic acid (H3AsO4) is a triprotic weak acid with the Ka values shown below. Solid sodium…

A: The acid dissociation constant is the measure of the extent up to which acid can deprotonate. The…

Q: What is the pOH of a 0.76 M solution of citric acid, if Ka = 7.4 x 10-4 of HC6H7O7.

A: Weak acids are not completely dissociated into ions in an aqueous solution. So, when it is dissolved…

Q: The pH of a 0.94M solution of hydrofluoric acid (HF) is measured to be 1.60. Calculate the acid…

A:

Q: The pH of a weak acid can be approximated by the equation: The graph below shows a plot of pH…

A: Answer: When a weak acid is dissolved in water, it ionizes partially and there is an equilibrium…

Q: Define pKa for a weak acid. What is the relationship between the value of the pKa and the strength…

A:

Q: Saccharin is a monoprotic acid. If the pH of a 6.30 x 10–3 M solution of this acid is 5.63, what is…

A: The dissociation of saccharin is given as, HSac↔H+ + Sac- By definition, the acid dissociation…

Q: Based on their compositions and structures and on conjugate acid–base relationships, select the…

A: The species formed after the acid donates a proton is termed as a Conjugate base. The species formed…

Q: The acid-dissociation constant, Ka, for gallic acid is 4.57x10-3. What is the base-dissociation…

A: Base dissociation constant is a constant which occur at the equilibrium in which base reacts with…

Q: What is the percent ionization of a 0.36M aqueous solution of formic acid, HCHO2 that is also 0.08 M…

A: 0.36 M aqueous solution of formic acid is present in 0.08 M HCl. The Ka of formic acid is 1.7 * 10-4…

Q: 1.00 M solution of acetic acid, C2O2H4, has a pH of 2.30. a) Calculate the [H3O+], [OH-], Ka, Kb,…

A: “Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: In which of the following aqueous solutions does the weak acid exhibit the highest percentage…

A: Percentage ionization is given as: More Stronger the acid, More will be  [H+]

Q: Use the Ka values for the following acids to find the strongest conjugate base : HS O3- : 6.3 * 10 ^…

A: Answer:

Q: Complete the following table, which lists information about the measured acid dissociation constants…

A:

Q: The Ka for hydrofluoric acid is 6.8x10-4. What percentage of the HF is dissociated in a 0.08M…

A: Hydrofluoric acid is a weak acid that is very slowly dissociate to give H+ and F-. So, for…

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.