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 buffer solution is 0.316 M in CH;COOH and 0.275 M in CH3COON . If K, for CH;COOH is 1.8×10³ , what…

A: Concentration of CH3COOH=0.316M Concentration of CH3COONa=0.275M Ka of CH3COOH=1.8×10^-5 pH=?

Q: The pH of an aqueous solution of weak monoprotic acid is 3.15. What is the initial…

A: Value of pH is sued to measure acidity or basicity of a solution. Value of pH lies in the range from…

Q: A student has a sample of 0.50 M lactic acid (HC3H5O3). She adds 10 mL of this solution to 40 mL of…

A: Given : Concentration of lactic acid = 0.50 M Volume of lactic acid solution used = 10 mL = 0.010 L…

Q: You are studying a clear solution and you added the pH indicator methyl violet. The colour range of…

A: The color of a solution of pH 0.2 is needed to be determined on the addition of an acid-base…

Q: CoHsOH(ag) + H2O0 → CaHsO(aq) + H3O*@g K= 1.12 x 1010 (a) Phenol is a weak acid that partially…

A: Since you have asked a question with multiple parts, we are solving first three parts for you. For…

Q: A solution is made by dissolving 18.7 g of CH3NH:NO: in 500.0 mL of water. L Does CH.NH:- have any…

A: Given,  Mass of CH3NH3NO3 = 18.7 g.  Volume of water = 500.0 mL

Q: What is the pH of a solution that results from mixing together equal volumes of a 0.150 M solution…

A: Answer :

Q: In a 1.18 M  aqueous solution of a monoprotic acid, 3.81% of the acid is ionized. What is the value…

A: Acid dissociation constant ka is given by equilibrium concentration of product divided by…

Q: An acetic acid solution was prepared by dissolving 0.02 moles of acetic acid (HOAC) in water to give…

A: The detailed answer has been provided.

Q: A solution (total volume = 1L) of 0.4 M NH3 contains 12.78 g of NHẠCI (MW = 53.491 g/mol). Kb = 1.8…

A:

Q: Given 1.00 L of a solution that is 0.100 M in sodium propionate (NaC3H5O2) and 0.300 M in propionic…

A: A buffer is a solution which resist any change in pH on adding a small amount of acid or base . it…

Q: When 14.08 mL of 0.1594 M NaOH is added to 25.00 mL of 0.1235 M HX (an unknown weak acid), the…

A: Given, Volume of NaOH = 14.08 mL Molarity of NaOH = 0.1594 M Volume of unknown weak acid =25.00 mL…

Q: Calculate the pH of the following solutions. (1)Tap water after boiling       (2)  0.0010 M NaOH…

A: Note - Since you have asked a question with multiple sub-parts, we will do the first three sub-parts…

Q: A chemist adds a chemical to pure water and there is a 100-fold incre approximation of the new pH…

A: The objective of the question is to calculate the new .

Q: According to the table in the text, hydrogen fluoride (HF) has a pk, of 3.2. If a solution of HF is…

A:

Q: Calculate the pH change that results when 15 mL of 2.0 M HCI is added to 580. mL of each of the…

A: The objective of the question is to calculate the  change.

Q: aNH2

A: Generally, sodium amide (NaNH2) is a very good nucleophilic reagent as well as it is used as a base.…

Q: en 13.75 mL of a 1.074 M solution of KOH has been added to a 27.5 mL f hydrofluoric acid with a…

A: We will calculate pH

Q: In the laboratory, a general chemistry student measured the pH of a 0.429 M aqueous solution of…

A:

Q: Calculate the pH change that results when 15 mL of 2.0 M HCl is added to 560. mL of each of the…

A: The formula to calculate the pH is

Q: A student has a sample of 0.50 M lactic acid (HC 3H5O 3). She adds 10 mL of this solution to 40 mL…

A: The objective of the question is to write a chemical reaction for the dissociation of lactic acid in…

Q: A new potential cure for the common cold, code-named Z-123, is being tested by a pharmaceutical…

A:

Q: a value of 7.2 x 10*. What is the pH to 2 decimal -f hydrofluoric acid with a concentration of 0.537…

A: We will calculate pH

Q: . (a) Combine the following equations to construct an acid-base reaction equation, in the process…

A:

Q: An analytic chemist is titrating 65.9 mL od 0.4200 M solution of piperidine (C6N10NH) with a 0.8800…

A: First calculate the number of moles for both given base and acid. Then use that moles to find out…

Q: None

A: (b) Addition of 3.00 mL of 0.500 M NaOH to 30.0 mL of buffer:Given pH: 8.13(c) Addition of 15.0 mL…

Q: Given that Ka’s for hydrofluoric acid (HF) and boric acid (H3BO3) are 6.3 × 10^–4and 5.4 × 10^–10,…

A: a) Given: Volume of HF=50 mL Concentration of HF= 0.2 M Concentration of NaH2BO3= 0.5 M Volume of…

Q: In the laboratory, a general chemistry student measured the pH of a 0.365 M aqueous solution of…

A: Hello. Since your question has multiple parts, we will solve the first question for you. If you want…

Q: A 1.0 M solution of a weak acid, HA has a pH of 2.64. What is the value of Ka for this acid?

A: The acidic strength of all known acids is dependent on their dissociation constants. This constant…

Q: Calculate the acetate ion concentration in a solution prepared by dissolving 8.70×10-3 mol of HCl(g)…

A: First calculate molarity of HCl concentration of acetate Ion use √Ka×C HCL is a strong acid while…

Q: 3c.) Suppose it is desired to maintain the pH of a solution at 4.2 using only acetic acid and sodium…

A: We have to tell which option is correct from given choices of options

Q: (a) Using the expression Ka=[H+][A−]/[HA], explain how to determine which solution has the lower pH,…

A:

Q: Calculate the pH change that results when 14 mL of 2.4 M HCl is added to 510. mL of each of the…

A:

Q: What is the pH of a solution that is 0.29 M KOCN and 0.14 M HOCN (cyanic acid)? (Ka for HOCN is…

A: Hensderson equation for the calculation of pH of a buffer solution consisting of a solution of weak…

Q: The pH of 0.800 M aqueous benzenesulfonic acid (a monoprotic acid) is 0.51. What is the value of Ka…

A:

Q: B. Calculate the pH after 17.50 mL of NaOH is added to 35.00 mL of acetic acid using the…

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.