5 g of cyanoacetic acid, CH2CNCOOH in a liter of aqueous solution has a pH of 1.89. what is the value of ka?

Q: A 0.110 M solution of an unknown weak acid has a pH of 4.35 at 25 degrees celsius. What is the…

A: The concentration of hydronium ion in solution can be calculated by using PH equation Ka for weak…

Q: A solution of 0.20 M hydrazoic acid has a pH of 3.21. What is the Ka of hydrazoic acid?

A: We have to calculate the Ka of acid.

Q: Carbon dioxide in the atmosphere dissolves in raindrops toproduce carbonic acid (H2CO3), causing the…

A: To find the range of [H+] and [OH-] in the raindrops can be given by- Since, Product of the both…

Q: Calculate the concentration of OH and the pH of a solution that is 0.20 M in aqueous NH3 and 0.10 M…

A: This is basic buffer question.

Q: A 0.17 M solution of a weak acid has a pH of 2.85. What is the ka of the weak acid?

A: Given: concentration of weak acid=0.17M              pH of weak acid=2.85 To calculate: Ka of weak…

Q: Phenylacetic acid, HC8H7O2, is one of the substances that accumulates in the blood of persons with…

A: According to the question, we have 0.0950 M solution of Phenylacetic acid that has a pH of 2.75.…

Q: 69. A 0.185 M solution of a weak acid (HA) has a pH of 2.95. Calcu- late the acid ionization…

A: For weak acid : pH = 1/2pKa-1/2logC  Or, pKa = 2pH+logC ...(1)  Here, pH = 2.95 and C = 0.185 M…

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: What is the pH of a solution obtained by dissolving two extra-strength aspirin tablets, containing…

A: Acetylsalicylic acid, commonly known as aspirin is a most widely used medicine for reducing pain,…

Q: Aspirin, a drug that is used to relieve minor aches and pain, is a weak monoprotic acid. What is the…

A: we know that pH = -log [H+] so -log [H+] = 3.12 [H+] = 0.000758

Q: Calculate the pH of a solution prepared by dissolving 5.00 g of NaCIO in 400.0 mL of water.

A: Mass of NaClO  = 5.00g Volume of solution = 400.0 mL=400 ×10-3L Ka = 2.9 × 10-8

Q: In a solution prepared by dissolving 0.100 mole of propanoic acid in enough water to make 1.00 L of…

A:

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: What are the concentrations of hydrogen ion and hydroxide ion in household ammonia, an aqueous…

A: The hydrogen ion concentration in aqueous solution of NH3 is calculated as shown below. on…

Q: If the Ka of a monoprotic weak acid is 3.7×10−6, what is the pH of a 0.39 M solution of this acid?

A:

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: A 0.15 M solution of an acid found in milk has a pH of 2.80. What is the percentage ionization of…

A: HA → H+ + A- The formula to calculate the pH is, pH= -log[H+] Therefore rearranging the formula let…

Q: What is the pH of a 0.30 M solution of methylammonium chloride, CH3NH3CL?  What is the…

A:

Q: The Ka of a weak monoprotic acid is 1.13 × 10−5 . What is the pH of a 0.0885 M solution of this…

A:

Q: A typical aspirin tablet contains 325 mg of acetylsalicylic acid, HC9H7O4. Calculate the pH of a…

A: Calculate the concentration of aspirin solution: 1 mg = 0.001 g 1 mL = 0.001 L

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: The acetate ion is the conjugate base of acetic acid. The Ka of acetic acid is 1.76×10–5 What is…

A: Given: The Ka (acid dissociation constant) value of acetic acid is 1.76 x 10-5 The molarity of…

Q: When the conjugate base of a weak acid (in the form of a salt) is dissolved in water, one can…

A: As we know that water is neither acidic nor basic and it is neutral in nature. We also know that…

Q: 7. The ka for acetic acid is 1.0 x 10.5. Is acetic acid a weak or a strong acid?

A: Strong acids completely dissociate in aqueous solution (Ka > 1, pKa < 1).

Q: Saccharin, a sugar substitute, is a weak acid with pKa = 2.32at 25 °C. It ionizes in aqueous…

A: Since the reaction given is HNC7H4SO3(aq) ⇌ H+(aq) +HNC7H4SO3-(aq) hence assuming that y…

Q: If the ph of 0.10 M HA (weak acid) is 4.10, calculate Ka for this weak acid.

A: From given pH value the hydronium ion concentration is determined first.

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: Which of the following is the pH of the solution containing 0.01 mol CH3COOH and 0.820 grams of…

A: Use the Henderson-Hasselbalch equation, which I have shown below: pH = pKa + log [[CH3COO-]…

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: A 0.115 M solution of a weak acid (HA) has a pH of 3.29. Calculate the acid ionization constant (Ka)…

A: The concentration of HA = 0.115 M pH = 3.29 pH = 3.29H3O+ =10-pH=10-3.29=0.000513 M

Q: The value of Ka for acetic acid is 1.75 × 10—5. The pH of a 0.100 M solution of acetic acid is:

A:

Q: 1. Calculate the pH of a solution prepared by dissolving 2.13 g of picric acid, (NO2);C6H2OH (229.11…

A:

Q: A typical aspirin tablet contains 325 mg acetylsalicylic acid. Calculate the pH of a solution that…

A:

Q: What is the Ka of a weak acid whose 0.10 M solution produces a pH of 2.38?

A:

Q: The acetate ion is the conjugate base of acetic acid. The Ka of acetic acid is 1.76×10–5. What is…

A: Sodium acetate is a salt of weak acid (CH3COOH) and strong base(NaOH).CH3COONa →  CH3COO- +…

Q: The hydroxide ion (OH-) concentration in skim milk was measured to be  5.4 x 10-8 M. What is the pH…

A:

Q: What is the Ka of bromoacetic acid if a 0.035 M bromoacetic acid aqueous solution has a pH of 2.22?

A: Let us take a reaction,        HX = H+ + X-  The dissociation constant of the above reaction is,  Ka…

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: 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: a) A 0.10 Maqueous solution of propanoic acid, CH3CH2COOH, has a pH of 2.93. What is the value of…

A: Hi since you have posted multiple questions, we will answer the very first question. Kindly repost…

Q: The pH of a 0.220M solution of a weak acid, HB, is 2.51. What is Ka for the weak acid?

A: Given  PH of weak acid = 2.51  Concentration of weak acid ( c ) = 0.220 M  Ionization constant ( Ka…

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: The acetate ion is the conjugate base of acetic acid. The Ka of acetic acid is 1.76×10–5. What is…

A: Kb for the acetate ion is determined as follows,

Q: The pH of a 0.16 M solution of a weak acid, HA, is 2.85. What is the value of Ka for the weak acid?

A: The question is based on the dissociation of weak electrolyte. We  have been given a weak Acid which…

Q: Calculate the pH of a solution that is 0.450 M HC2H2O2 and 0.730 M NaC2H3O2. The Ka for acetic acid…

A: This problem is solved by using Henderson Hassel baltch equation.

Q: What is the Ka of hydrazoic acid if a 0.020 M hydrazoic acid aqueous solution has a pH of 3.22?

A:

Q: Sodium ascorbate is the sodium salt of ascorbic acid (i.e. Vitamin C) and is used as an antioxidant…

A: We have to predict the pH of 0.15 M solution for ascorbate ion.

Q: The pH of a 0.800 M aqueous solution of a weak acid is 1.99. What is the value of Ka for this acid?

A: Given  pH = 1.99 Concentration (c) = 0.800 M Ka =?

Q: Sodium benzoate (NaC6H5COO) is a common food preservative. What is the pH of a 0.150 M NaC6H5COO…

A:

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. 

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.