4. Write the Ka expression for each of the following in water: а. HNO b. CH3COOH c. HBRO2

Q: What is the pH of a solution containing the following: a. 80 mM H* b. 2x10-2 mg/LH c. 6x10- mg/L OH

A: The solutions given are,

Q: Which will have the highest [OH-]? 1.0 M for all options below. a. CsCl b. KNO3 c. NH3 d. KCl…

A: Which will have the highest [OH-] ? 1.0 M for all options --

Q: 2. The weak acid HCN establishes an equilibrium with its ions when dissolved in water. HCN (aq) -→…

A: The reaction for dissociation of HCN is given by, HCN(aq) ⇔ H+(aq) + CN-(aq) When KCN is added, it…

Q: All of the following are weak bases except:  A. Al(OH)3 B. Mg(OH)2 C. NH3 D. B(OH)3

A: The compound that is weak base has to be identified.

Q: bioo avinsdoni 14. Which of the following binary acid would have the largest acid dissociation…

A: The acid dissociation constant, Ka, is a measure of the strength of an acid in solution. It is the…

Q: Of the following acids, does not require an ICE table to determine solution pH. Select one: O A.…

A: Given acids: H2CO3, HBr, HF, HClO, HNO2 We have to find which one of them does not require an ICE…

Q: QUESTION 16 A salt will dissolve in water to form O a. bases O b. acids Oc. buffers d. jons other…

A: salt is formed by the neutralization reaction  between any acid and base when  an acid (HX ) react…

Q: Match: Substance Definition Lewis acid A. Provides H in water Bronsted-Lowry base B. Provides OH in…

A: According to the Lewis concept the species which accept a lone pair of electrons known as Lewis…

Q: Cinnamaldehyde, the aromatic constituent of cinnamon oil, can be synthesized by a mix aldol-like…

A:

Q: 4. Calculate the value of [H3O*]and [OH] in each solution: a. 0.0001 M NaOH b. 0.0001 M HCI

A: 4. Given,a. 0.0001 M NaOHb. 0.0001 M HClRequired,                     The value of H3O+ and OH- .

Q: 2. The percent ionization of a weak acid: a. Decreases as molar concentration increases b. Stays the…

A: Divide the mass of the dissociated ions by the total mass of the dissociated and non-dissociated…

Q: The

A: Cl have more electronegative element than other so that it's Decreases the electrons charges density…

Q: = HA = H,O* = A %3D The strongest acid is: А. НХ В. HY С. HZ D. Not enough info HX HY HZ

A: Acidity is defined as tendency to release H+ in the water . As the no of H+ increase then acidity…

Q: The addition of a strong acid like HCI to an aqueous solution would result in O the release of H*…

A: HCl is strong acid . When it is dissolved in water , it will readily release H+ ion in aqueous…

Q: 10. Each of the following pairs contains one strong acid and one weak acid EXCEPT a. HF and HOCI b.…

A: According to the Arrhenius theory, the substances that give H+ ions when dissolved in water easily…

Q: You have a solution of NaCl. What effect will addition of NH,CI have on the pH of the solution? K,…

A: NaCl is a salt of strong acid and a strong base. So, it is a neutral salt. NH4Cl is a salt of strong…

Q: The 0.10 M solution with the lowest pH is: A. HC2H302(ac) B. NH3(ac) C. NaOH(ac) D. HNO3(ac) ??

A:

Q: When 50 mL of 0.20 M ammonium nitrate and 50 mL of 0.10 M calcium hydroxide are combined, the pH of…

A: Volume of ammonium nitrate solution= 50 mL  Concentration of ammonium nitrate solution = 0.20 M…

Q: Question 6 Predict whether a 0.10-M solution of each of the following salts will be basic, acidic,…

A: ->Salt of strong acid and weak base is acidic. ->Salt of weak acid and strong base is basic.…

Q: Write the Ka expression for each of the following in water: a HNO; b. CH.COOH HBrO

A: Here we are required to find the dissociation constant expression for acid given below

Q: A 0.33 M HF solution has a percent ionization of 0.47%. What is the H* ion concentration at…

A:

Q: Arrange the following in order of increasing AHfus- (1 being the lowest and 4 being the highest)…

A: Answer :

Q: 1.Calculate the molarity of the hydrogen ion for each of the following solutions: a. pOH = 4.99 b.…

A: Four numerical problems based on pH concept, which are to be accomplished.

Q: Write the ionization of the following substances: a. Ca(OH)2 b. H2CO3 c. HCO3-

A:

Q: 1. Write the Ka expression for each of the following in water: 2. H2РОД 3. HSO4 4. НОСI 5. NH4*

A: Ka is an equilibrium constant for acid , and an acid is a substance that gives a proton when…

Q: 34) Hypochlorus acid, HCI0, has a ha oF 3.0 x 10-8 q= Calculate hb For the hypochlorite ion %3D

A:

Q: A. 0.080 M HNO₂ B. 0.30 M NH 3 C. 1.5x10-8 M KOH D. 4.1x10-5 M HBr

A:

Q: 15. Knowing that Nitrogen and Oxygen compounds can combine in a variety of ratios, what is the name…

A:

Q: Ph, Ph-P: Ph Predict the product of this Wittig reaction : Ph. Ph (A) (В) (C) (D) Ph Ph Ph Ph H. Ph…

A: The reaction between ketone or aldehyde with triphenylphosphonium ylide produce a new alkene bond.…

Q: C. Me Me H cat. AcOH A, PhMe

A: Given reaction is an example of nucleophilic addition reaction of carbonyl carbon.

Q: Which of these acids is the strongest given these K₂ values ? Acid A, K₂ = 0.00054 - Acid B, K₂ =…

A: Given , the ka values we have to determine which acid is strongest

Q: If a 0.50 mol/L weak acid is diluted to 0.050 mol/L at constant temperature, which of the following…

A: Given, Initial concentration of weak acid H+ = 0.50 M  Diluted concentration of that acid H+ = 0.050…

Q: Which one of the following is a buffer solution?

A: Given question a some acid base compound is given . following compounds is a buffer solution.…

Q: Write the ionization equation and the Ka expression for each of the ff. acids. a. HSO3- b. HPO42- c.…

A: Ionization equation: Ionization can be defined as complete loss or gain of electrons in the aqueous…

Q: The weak acid HA is 10 % ionized (dissociated) in a 0.20 M solution. The Ka for this acid is:

A: Dissociation constant is a quantity that tells the extent to which a particular substance gets…

Q: You drink a liter of pure, neutral pH water. You have just consumed a. 10-7 moles OH- ions b. 10-7…

A: Since the pH of neutral water = 7  And since we know that  pH = 14 + log[OH-] = -log[H3O+] where…

Q: Categorize each of the following as either strong, weak, or nonelectrolytes: e. Agl₂ a. KF b. HCI c.…

A: a electrolyte that completely dissociates into its  ions in solution is called strong…

Q: Calculate the Ka of an acid, HX, whose ionization is 31% when CHX= 0.60 M (Note that the %…

A:

Q: Based on the given K, values, rank the following acids from strongest (1) to weakest (5). Carbonic…

A:

Q: The pH of four different solutions of common materials is measured. Which of the following lists the…

A: A multiple choice question about pH concept, which is to be accomplished.

Q: A 0.785M solution of the weak acid, hypoiodous acid, HOI, has a Ka of 2.32x10-11. What is the…

A: The concentration of weak acid (HA) = 0.785 M The equilibrium constant for the weak acid, Ka =…

Q: What is the Ka expression that can be derived from the ionization of HPO42- in water?

A: Equilibrium is the state of the reversible reactions. So when the rate of the forward direction…

Q: 4. Write the ionization equation and K expression for: + a. HC,H,O, b. NH, c. HCIO, d. HCO,

A:

Q: which two solutions have the lowest concentration of H+ ions? 1. window cleaner 2. detergent 3. HCl…

A: pH is the negative logarithm of H+ ion concentration.The concentration of H+ ions in a solution is…

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.