Consider the acid HXOy where X is a halogen that is less electronegative than oxygen. Which of the following gives the relationship between Ka of the acid and the value of y and gives the correct reasoning? As y increases the value of Ka increases because the conjugate base of the acid becomes less stable. As y increases the value of Ka increases because the conjugate base of the acid becomes more stable. As y increases the value of Ka decreases because the conjugate base of the acid becomes less stable. As y increases the value of Ka decreases because the conjugate base of the acid becomes more stable.

Q: Consider the following acidic equilibrium: H₂CO3(aq) + H₂O(1) HCO3(aq) + H3O*(aq). If you add NaHCO3…

A: According to Le-Chatelier's principle, if the equilibrium reaction is disturbed by changing…

Q: Determine the Ka of an acid whose 0.294 M solution has a pH of 2.80. 4.3 x 10-4 ○ 8.6 x 10-6 O 4.9 x…

A: The problem is asking us to find the Ka, or acid dissociation constant, of an acid. The Ka is a…

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 0.00959 M solution of a weak base has a pH of 9.33. What is the Ka for its conjugate acid?

A: Concentration of OH- is calculated as follows,

Q: True or False: To find the pH of a weak base solution, you must calculate the equilibrium…

A: Weak bases are those substances which dissociate partially in the solution producing OH- ions in the…

Q: Consider the following chemical reaction and that H2SO4 is a strong acid: H2SO4 + H2O ==== HSO4- +…

A:

Q: A solution is made by dissolving 13.9 g of HONH:CIO3 in 500.0 mL of water. Does CIOS- have any…

A:

Q: When 0.075 mol of propionic acid, C2H5CO2H, is dissolved in 400 mL of water, the equilibrium…

A: The concentration of propionic acid and the ions has to be calculated in order to obtain the Ka.

Q: highlighted reactant reaction Bronsted-Lowry Bronsted-Lowry base neither acid HBr(aq) + OH (aq) → Br…

A: Bronsted Lowry base: a proton acceptor Bronsted Lowry acid : a proton donor

Q: A 0.54 M solution of chloroacetic acid, CICH2 CO2H, has a pH of 1.57. Calculate K, for the acid. %3D

A: Given: The molarity of the solution of chloroacetic acid = 0.54 M The pH of the solution = 1.57 We…

Q: Nitrous Acid (HNO2) has a Ka value of 5.6x10–4. Calculate the pH of a solution that is 0.00298 M…

A: pH = -log[H+] For a weak acid solution: [H+] = (Ka x C)1/2 Where, C = molarity of acid

Q: A 2.0 L solution made by adding solid NaClO to water resulted in a basic equilibrium with a pH of…

A:

Q: Calculate the acid ionization constant (pKa) for the acid with a 0.775 M solution of a weak acid…

A: Given data of the following:: [weak acid] = 0.775 M = [HA]  pH = 3.38 pka = ?

Q: What is the Ka of the acid in a solution that is 0.34 M in the acid, and 0.247 M in the conjugate…

A:

Q: A solution is prepared from two weak acids, 0.2 M HA and 0.1 M HB. If the Ka of HA is 1x10-5 and the…

A: pH - It is the negative logarithm of the hydronium ion concentration of a  solution. Equilibrium -…

Q: 7. What are the conjugate base and conjugate acid for HSO, ? What is the term used to describe…

A: Conjugate acid is formed when we add protons to a base and conjugate base is formed when proton is…

Q: Calculate the pH of a solution that is 1.00 M HClO and 0.50 M NaClO.

A: NaClO is salt of weak acid HClO and strong base NaOH.Therefore it forms a buffer solution ,whose pH…

Q: Heroin, a derivative of morphine, is a powerful analgesic and a powerful narcotic agent. Calculate…

A: Heroine is a base.

Q: acidic equilibrium

A:

Q: Explain why the neutralization reaction of a weak acid and a strong base gives a weakly basic…

A: the neutralization reaction is the reaction in which the acid and base react with each other to form…

Q: Ca(NO3)2 will be more soluble in

A: In its anhydrous form, calcium nitrate is readily soluble in water, equivalent to a solubility of…

Q: Which of the following salts, when dissolved in water, would produce a solution that is slightly…

A:

Q: If the Ka for a weak acid, HA, is 4.5 × 10−6, what is the Kb for its conjugate base, A−?

A:

Q: Acetic acid,  CH3COOH , has a  Ka of  1.8×10−5. Calculate  Kb  for the acetate ion.

A: Given, Ka for Acetic acid = 1.8 × 10-5 Kb for acetate ion = ? Note:  Kw = 1.0 × 10-14

Q: Determine the Ka of an acid whose 0.294 M solution has a pH of 2.80.

A: In this problem, we are asked to find the Ka (acid dissociation constant) of an acid. We are given…

Q: weak base that

A: Given that.  Concentration of weak base, and pKb

Q: A 0.120 M solution of a weak acid (HA ) has a pH of 3.26. Calculate the acid ionization constant…

A: The objective of this question is to calculate the acid ionization constant (Ka) for a weak acid…

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

A:

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: An acid has an initial concentration of 3.87×10−5. The pH of the solution, at equilibrium is 4.41.…

A: The reaction between pH, Ka and concentration of a solution is given as: pH=12pKa-12logc Here Ka is…

Q: The lower the pH of a weak acid, the: o higher the dissolved H2) concentration. o higher the acid…

A: lower the pH the weak acid has ?

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: contains

A:

Q: What is the concentration of H3O+ in a solution that is 0.0600 M Hypochlorous acid (HClO)? What is…

A: According to the question,  We need to calculate the concentration of H3O+ in a solution that is…

Q: Which of the following K values would indicate the weakest base of the group? O 1.2 x 109 O 6.3 x…

A: Ans:- (1.2×10-9 is the weakest base of the group).

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".