A 0.20 M solution of niacin has a pH of 3.6. (a) What percentage of the acid is ionized in this solution? (b) What is the Ka for niacin?

Q: The pH of a 0.50 M solution of an acid, HA, is 4.67. Calculate Ka of HA.

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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: 1) A 0.45M aqueous solutionof creatine, (C4H9N3O2), has a pH of 1.49. Calculate the value of the…

A:

Q: Calculate the pH of a 2.44 M HCIO3 solution. Ka for this acid is 1.5x10³. HCIO3 is a weak acid.

A:

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: 8) A 0.185 M solution of a weak acid has a pH of 2.95. Calculate the acid ionization constant (Ka)…

A: A 0.185 M solution of a weak acid (HA) has a pH of 2.95. Calculate the acid ionization constant Ka…

Q: Ethylammonium chloride, CH;CH;NH3CI, is an acidic salt. (i) Write equations to show the dissolving…

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Q: A 0.495M solution of nitrous acid, HNO2, has a pH of 1.83. Calculate the value of Ka for nitrous…

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Q: Write the chemical equation and the Ka expression for theionization of each of the following acids…

A: a)  HBrO2 l → H+ aq +BrO2- aqand writing the Ka expression :Ka=H+ BrO2-HBrO2The reaction to…

Q: 1) Calculate the pH (aq., 25 °C) of a 0.073 M Novocaine (C13H21O2N2CI) solution, which is the salt…

A: Solving only first question in accordance with guidelines. We will first draw ICE table and then…

Q: A 0.120 M solution of a weak acid (HA) has a pH of 3.29.  a) Calculate the acid ionization constant…

A: Given,Concentration of a solution of weak acid, HA = 0.120 MpH of the solution = 3.29The…

Q: Write the net ionic equation for the hydrolysis reaction that occurs when sodium carbonate, Na,CO3…

A: When sodium carbonate is made to react with water, it gives sodium bicarbonate and sodium…

Q: Calculate the pKa of the weak acid HA, given that a solution of 0.65 M HA and 0.85 M NaA has a pH of…

A: The formula for calculating pKa of an acid with the given values of pH and concentrations of HA and…

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

A:

Q: calculate the pH of the solution eith an H+1 concentration of 2.90×10-12 and identify the solution…

A: Given,  The concentration of H+ = 2.90 × 10-12 M The pH of the solution is:

Q: Calculate the pH of a .10 M solution of formic acid (HCHO2). The Ka of formic acid is 1.8 x 10-4.

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Q: In the laboratory, a general chemistry student measured the pH of a 0.578 M aqueous solution of…

A: For a weak acid, we have       pH = 1/2(pKa - logA) where A is the concentration of the acid. Given,…

Q: a general chemistry student measured the pH of a 0.510 M aqueous solution of nitrous acid to be…

A: Here we are required to find the dissociation constant for weak acid nitrous acid

Q: Formulate the acid-base reactions with ions, mark conjugate acid-base pairs of the reaction of…

A: Note- The product formed is ethyne and not ethene. Chemical formula of calcium carbide- CaC2…

Q: What is the pH in a 0.0320 M aqueous solution of formic acid (HCOOH)? (For HCOOH, Ka=1.8 x 10–4)

A: HCOOH is a weak organic acid. It dissociates into formate ions and hydrogen ions. The ICE table for…

Q: the pH of an acid solution is 3.59. If the concentration of the acid in the solution is 0.200 mol/L,…

A: Given Concentration of the acid=0.2 mol/LpH of the acid solution=3.59Ka of thel acid=??

Q: Calculate the pH of a solution prepared by dissolving 0.37 mol of formic acid (HCO2H) and 0.23 mol…

A: Given, moles of formic acid = 0.37 mol  moles of Sodium formate = 0.23 mol  Volume = 1 liter As we…

Q: Calculate the acid ionization constant (Ka) if the pH of the 0.1 M acetic acid solution is 2.87?

A: We have given that  Concentration of acetic acid = 0.1M  pH = 2.87

Q: For a weak acid, when does the pH equal the pKa?

A: Answer: For this we need to know Henderson-Hasselbalch equation . Explanation:…

Q: The pH of a 0.0492 M solution of a weak acid is 2.641. What is the Ka of the acid?

A: pH= 2.641

Q: Calculate the pH of a 0.20 M solution of sodium acetate (NaCH3COO) given that the Ka of acetic acid…

A:

Q: Calculate the pH of a 2.61 mol/L solution of ammonium hydrogen carbonate, NH4HCO3

A:

Q: substance with a pH of 2 is?

A:

Q: Predict the position of equilibrium and calculate the equilibrium constant, Keq, for   acid-base…

A: We know that strong acids will donate protons easily and strong base will accept proton easily. That…

Q: Write the Ka (acid ionization equilibrium constant) expression for the ionization of HC3H5O2 in…

A: Let us consider a general reaction for the ionization of an acid HA in water. HA (aq)  ↔ H+(aq) +…

Q: Calculate the pH of the following solutions: a. 0.34 M hydrocyanic acid. b. 1.5 M solution of…

A: pKa of hydrocyanic acid is 9.2

Q: If enough of a monoprotic acid is dissolved in water to produce a 0.0122 M solution with a pH of…

A: The dissociation of a monoprotic acid is represented as follows: HA(aq)+H2O(l) ↔ H3O+(aq)+A-(aq)…

Q: Calculate the pH of a solution prepared by dissolving 0.150 mol of acetic acid and 0.300 mol of…

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Q: Calculate the pH of a 0.50 M solution of sodium formate (NaHCOO) given that the Ka of formic acid…

A: Given,  The pH of a 0.50 M solution of sodium formate (NaCOOH) is: The Ka of formic acid (HCOOH) is…

Q: Define the equilibrium constant Ka (1.3 × 10–2) for the dissociation of the weak acid, HSO4–. Assume…

A:

Q: Based on the pH measured for the solution of (NH4)2CO3, is NH4+ is a stronger acid or is CO2−3…

A: Given: To determine whether (NH4)2CO3  is strong acid or strong base.   Definition: (NH4)2CO3 is…

Q: What is the pH of the following solution? Hydrogen sulphide is a weak acid and has a pka of 8.9 x…

A: Please be noted that the value given for H2S is Ka not pKa. Therefore, pKa(H2S)=8.9×10-8.

Q: At what pH is the concentration of a compound, with a pKa = 3.7, 10 times greater in its acidic form…

A: Given information: pKa = 3.7 [Acid] = 10[Base]

Q: The sodium salt of propanoic acid, NaCH3CH2CO2, is used as an antifungal agent by veterinarians.…

A: Given: The Kb for CH3CH2CO2- = 7.7 × 10-10 We have to calculate the concentrations of H3O+ and OH-,…

Q: A solution was prepared by 0.250 moles of ammonium chloride to 500.0 mL of 0.35 M ammonia. Given the…

A: For NH3 , pKb = -log Kb = -log ( 1.86 x 10-5 ) = 5 - log 1.86 = 5 - 0.27 = 4.73 Concentration of…

Q: Calculate the [H+] and pH of a 2.35×10−4 M hydrazoic acid solution. The Ka of hydrazoic acid is…

A: We wil use concept of weak acid for H+ and pH.

Q: Calculate the pH of a solution that is 0.195M in sodium formate (NaHCO2) and 0.24 M in formic acid…

A: Given: Concentration of  sodium formate (NaHCO2) = 0.195 M            formic acid (HCO2H)  = 0.24M…

Q: A 2.00 L aqueous solution of a monoprotic weak acid, HA, with a concentration of 0.105 M has a pH of…

A: Since pH = -log[H+] = -log[H3O+] Hence substituting the values we get  2 = -log[H3O+] => [H3O+] =…

Q: Calculate the pH and pOH for the following: a. 10mg of cyanic acid (pKa=9.21) in 1L of water

A:

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: 2.44 moles of HNO3 is added to water and the final volume is 330mL. The pH of this solution was…

A: Nitric acid is strong acid. Given , pH = 1.47

Q: How many moles of (CH3)3N  would need to be added to 459.2 mL of a 0.25 M solution of (CH3)3NHCL  to…

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: A 0.255 M solution of a weak acid, HA, has a pH of 3.24. Calculate the Ka for the acid.

A: For a weak acid solution: From the Ostwald's Law: [H+] = (Ka x C)1/2 pH = -log [H+]

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.