A 2.5 M solution of a weak acid, HA, is 1.8% ionized in water. What is the K, value for this weak acid?

Q: A weak acid, HA, has a p?apKa of 4.5424.542. If a solution of this acid has a pH of 4.4944.494, what…

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Q: weak monoprotic acid (HA) has an acid ionization constant Ka = 1.8x10° at 298 K. If 100 mL of a 0.10…

A: First write equilibrium equation for reaction of weak acid and strong base and fine limiting…

Q: What mass of HI must be present in 0.250 L of solution to obtain a solution with each pH value?a. pH…

A: Given, volume of solution = 0.250 L HI is a strong electrolyte and it ionizes in solution as,…

Q: What is the pH of a 40.0 mL solution that is 0.19 M in CN and 0.25 M in HCN? The K, for HCN is 4.9 x…

A: HCN ---- > H+ + CN-  Assuming y concentration of HCN is dissociated from the above reaction…

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: Given, [HA] = 0.15M pH = 2.80

Q: A 0.035 M solution of a weak acid (HA) has a pH of 4.88.What is the Kₐ of the acid?

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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: Given: concentration of acid = 0.15 M pH of solution = 2.80

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: A solution is prepared by adding 0.10 mol of ammonium chloride, NH4Cl, to 1.00 L of water.  Which…

A: Salt formed from Strong acid + Strong base gives neutral solutiom Strong acid + weak base gives…

Q: What is the equilibrium pH of an initially 0.37 M solution of a weak acid HA at 25°C? Ka = 4.89 x 10…

A: Acid dissociation constant Ka is utilized to determine the acidic and basic nature of a solution. It…

Q: What is the pH of a 0.677 M weak base solution? The K_{b} of the weak base is 0.000017.

A: we need to calculate the pH  0.677 M weak base solution

Q: The compound ammonia, NH3, is a weak base when dissolved in water. Write the K, expression for the…

A: The answer to the following question is given as:

Q: 4. A 0.020 M weak acid HA, has a pH of 3.21. What is the Ka of the acid?

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Q: What is the acid-ionization constant, Ka, for this acid?

A: Given data contains, Concentration of HA is 0.200 M. pH is 2.210. The given chemical equation is,…

Q: If the K, of a monoprotic weak acid is 7.5 x 10, what is the pH of a 0.42 M solution of this acid?…

A: Given: Ka=7.5×10-6 C=0.42M

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: What is the value of Ka of this acid? What is the percent ionization of this acid?

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Q: A 0.010 M aqueous solution of a weak acid HA has a pH of 4.0. What is the degree of ionization of HA…

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Q: The compound dimethylamine, (CH3),NH, is a weak base when dissolved in water. Write the K expression…

A: The ionization of weak base can be given by, Where B is the weak base and HB+ is its conjugate…

Q: A solution is made by dissolving 48.9 g of Ba(NO2)2 in 500.0 mL of water. As NO2¯ is a base, write…

A: Answer:- This question is answered by using the simple concept of hydrolysis of salt of weak acid…

Q: What is pOH of aqueous solution at 25 degrees that contains 3.98 *10^-9 M hydronium ion

A: The pH of a solution is given by: pH=-log[H3O+]                                       ...... (1)…

Q: Which solution is most acidic (that is, has the lowest pH)?(a) 1.0 M HCl(b) 2.0 M HF(c) A solution…

A: In order to solve this question, we will be using the formula of pH relating with pKa and log[c] for…

Q: What is the hydroxide ion, pH, and pOH of a solution with a hydrogen ion concentration of 3.25 x…

A: Given:  [H+] = 3.25 x 10-3 M  Kw = 10-14    Since [H+] < 10-7 M so solution is acidic in nature.…

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: Classify these salts as acidic, basic, or neutral. Acidic Basic Neutral NH,Br KCI K,CO, Na,S LİCIO,

A: Salt is formed as the product of the neutralization reaction between an acid and a base. The salts…

Q: An acid (HA) dissociates as follows: HA - H* + A minus Arrow should be interpreted as an equilibrium…

A: An acid is a particular substance which upon dissociation in an aqueous medium gives H+ ions…

Q: Which would have a higher pH, a solution whose pOH is 5.00 or a solution whose hydrogen ion…

A: pH of solution is calculated based on the hydrogen ion concentration. pH = -log[H+] pH = 14 - pOH

Q: Calculate the concentration at which a monoprotic acid with K, = 3.0 x 10 will be 1.6% ionized.

A: Dissociation constant (K) - In dissociation reaction, ratio of concentration of product (dissociated…

Q: List the acidic salts in increasing order of acid strength, then list the basic salts in increasing…

A: Acid are the substance which donates proton in the aqueous solution. Example:HCl(aq)→H+(aq)+Cl-(aq)…

Q: 2b.For each of the following salts indicate whether the aqueous solution will be acidic basic or…

A: The acidity or basicity of a salt can be determined by its dissociation. If salt is formed from a…

Q: A chemist makes a 1.0 L of a solution that is both 0.6 M NH, and 0.8 M NH,CI. pK, of NH3 = 4.75.…

A: Given :-  Concentration of NH3 solution = 0.6 M  Concentration of NH4Cl = 0.8 M  Volume = 1 L  pKb…

Q: 6) A 0.25M solution of a CH,NH, has a pH of 10.25. a) Write the K, reaction for CH;NH2. b) Calculate…

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Q: Calculate [H+] for each of the following solutions, andindicate whether the solution is acidic,…

A: pH = -log[H+] pOH = -log [OH-] pH + pOH = 14

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: Which of the following statements about acids is true? O All of the other statements are false O For…

A: The question is based on the concept of equilibrium.    it involves calculation of hydronium ion…

Q: The following diagrams represent aqueous solutions of two HX HY monoprotic acids, HX and HY. The…

A: From given diagram We are determinining *stronger acid *stronger base *equilibrium shift when HX and…

Q: Calculate the equilibrium concentration of the nonionized bases and all ions in a solution that is…

A: Given that: concentration of NH3 = 0.115 M concentration of C6H5NH2 =  0.100 M To find:…

Q: A 0.80 M solution of Carbonic acid is prepared and is in equilibrium with its ions. The chemical…

A: Given data Initial concentration : 0.8 M Ionization constant : Ka=4.3×10-7 Equilibrium reaction…

Q: Fill in the blanks. When an acid is added to pure water the increases and the decreases. O A) H30*…

A: An acid is a substance which increases concentration of H3O+ in solution. Note :- acid has pH<7…

Q: What is the pH of a solution in which 15 mL of 0.15 M NaOH is added to 25 mL of a 0.10 M HCl ?

A: HCl is a strong acid and NaOH is a strong base. The net ionic equation involved in the titration of…

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 OH concentration and pH of a 1.8 x 10 M aqueous solution of sodium cyanide, NACN.…

A: Given: [NaCN(aq)] = 1.8 × 10-3 ,Ka = 4.9 × 10-10 Given reaction: NaCN(aq)    ---> Na+ (aq) +…

Q: A certain weak acid, HA, has a K, value of 4.6x10-7. Percent ionization for a weak acid (HA) is…

A: Answer: When a weak acid is added in water, its partial ionization takes place whose degree depends…

Q: A chemist makes a new solution: 1.0 L of a solution that is both that is both 0.6 M NH, and 0.8 M…

A: NH3 and NH4Cl make a basic buffer solution because NH3 is weak base and NH4Cl is strong acid salt

Q: 1. Which solution has the lowest pH? A. 0.10 M HCIO, В. О.10 М НСО C. 0.10 M KOH D. 0.10 M CH,NH;

A: The pH of the solution depends upon the negative logarithm of hydrogen ion concentration and written…

Q: what do you expect to happen to the pH of the same if you add 1 ml of i M NaOH instead of 1 ml of 1…

A: Answer PH  does not effect by adding acid or base in the system 1ml of…

Q: what do you expect to happen to the pH of the same if you add 11 ml of i M NaOH instead of 11 ml of…

A: 1st it depends on the solution where you are adding it.  for example, if the original solution is…

Q: The Kb of C6H5NH3+ is 3.98x10-10 1. What is its Ka? 2. What is the [H3O+] concentration in a…

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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.