14. When 0.1 mol of a salt is dissolved in 1.0 L of solution, the pH of the solution is 8.07. What is the identity of the salt? (a) NaF (b) NH.C1 (c) NaCl (d) КОН

Q: Citric acid, which is present in citrus fruits, is a triprotic acid. (a) Calculate the pH of a 0.040…

A: Citric acid- It is weak organic acid. Dissociate in water as,

Q: Liquid ammonia autoionizes like water:2NH₃(l) →NH₄⁺(am)+NH₂⁻(am) where (am) represents…

A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: Predict the pH (>7, <7, OR =7) of aqueous solutions containing the following salts: (a) KBr (b)…

A: (a) KBr is formed from neutralization of strong acid and strong base. On dissolution in water, the…

Q: A solution is made by dissolving 43.5 g of Ba(NO₂)2 in 500.0 mL of water. (a).As NO₂ is a base,…

A:

Q: Propionic acid, HC3H5O2, has Ka= 1.34 x 10–5. (a) What is the molar concentration of H3O+ in 0.15 M…

A: HC3H5O2 is a weak acid and dissociates in aqueous solution as: HC3H5O2+H2O↔C3H5O2-+H3O+

Q: The pH of a 0.1 M solution of a monobasic acid P is 1.0 while the pH of a 0.2 M solution of another…

A: Here we have to explain the properties the two monobasic acid P and Q . Given - The pH of 0.1 M P is…

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: Rank the compounds in each of the following groups in order of increasing acidity or basicity, as…

A: a) HCl &lt; HBr &lt; HI  b) H2O &lt; Cl- &lt; OH- &lt; H-

Q: Don’t ever mix acid with cyanide (CN) because it liberates poisonous HCN(g). But, just for fun,…

A: (a)

Q: 19.00 mL of 0.100 M sodium hydroxide is added to 39.00 mL of a 0.100 M acetic acid solution. The Ka…

A: Since sodium hydroxide is a strong base.  hence it will react with the acetic acid as  NaOH +…

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: The major component of vinegar is acetic acid, CH3COOH. Its Ka is 1.8 × 10-5 . One student used…

A: The question is based on the concept of titrations. We have to calculate molarity of the acid and Ph…

Q: Three beakers contain 100. mL of 0.10 M acid, either HCl,HClO₂, or HClO. (a) Find the pH of each.…

A: An acid furnishes the hydrogen ions in the aqueous solution. The stronger acid dissociates…

Q: Which are Lewis acids and which are Lewis bases?(a) Mg²⁺(b) OH⁻(c) SiF₄(d) BeCl₂

A:

Q: The sample of 25.0 mL of 0.0200 M NH3 is titrated with a 20.0 mL of 0.0150 M HCl solution. (a) Show…

A:

Q: (a) What is the pH of 0.75 M NaF?(b) What is the pH of 0.88 M pyridinium chloride, C₅H₅NHCl?

A: a) The pH of 0.75 M NaF is 8.52.

Q: Calculate the pOH and pH of a 0.0045 M solution of NaOH.

A: concentration of NaOH solution is 0.0045 M  we have to find pH and pOH of solution  pH = -log[H+]…

Q: 13. A 60.00 mL sample of 0.075 M sodium benzoate (NaC7H5O2) was titrated with 0.050 M HCl. What is…

A: Sodium benzoate is a salt and HCl is an acid.

Q: Calculate the pH of a solution containing 0.20 M CH3COOH and 0.30 M CH;COONA. [Ka CH3COOH = 1.8 x…

A:

Q: Hydrochloric acid is one of the common acids used in the laboratory. It is a very strong acid and…

A: Acid is a substance that releases H+ to the solution.  HCl dissociates almost completely in the…

Q: this is the complete question: What is the pH of the following mixtures? (a) 0.050 M NaHSO3 (b) 0.50…

A: Since your question has multiple sub-parts, we will answer the first three sub-parts for you. If you…

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: 4.Indicate whether the following solutions are acidic (A), basic (B), or neutral (N). (a)pH 8.6…

A: (a) pH = 8.6   The nature of solution can be determined from the pH scale as:   pH scale ranges from…

Q: - pH of Saliva The pH of saliva is normally in the range of 6.4 to 7.0. However, when a person is…

A: The acidic saliva indicates that the bacteria present in mouth breaks down the consumed carbohydrate…

Q: Calculate the pH of each of the following solutions. (a) 0.109 M HONH, (Kb = 1.1 × 10-8) 4.0 9.34 x…

A: The concentration of HONH2 = 0.109 M The concentration of HONH3+ = 0.109 M

Q: 25) Consider 0.14 M monoprotic acid (HA) that is 12% ionized. (a) Show the reaction of dissociation…

A:

Q: The acid dissociation constants for sulfurous acid are: Ka1 = 1.2 x 10-2 and Ka2 = 6.6 x 10-8 (a)…

A: Given, Acid dissociation constants of H2SO3 are: Ka1=1.2×10-2Ka2=6.6×10-8

Q: The ka of an unknown acid, HYO₂,  is determined to be 5 x 10⁻² empirically. What is the pH of a 0.1…

A: The objective of this question is to calculate the pH of a 0.1 M solution of an unknown acid HYO2,…

Q: We dissolve 2.66 g of an unknown acid, HA, in enough water to produce 25.0 mL of solution. The pH of…

A:

Q: Calcium propionate [Ca(CH₃CH₂COO)₂; calcium pro-panoate] is a mold inhibitor used in food, tobacco,…

A: The propionate ions (CH3CH2COO-) formed after dissociation of calcium propionate forms hydroxyl ions…

Q: 6. (a) Write an equation where calcium acetate is adding to water. (b) Looking at the equation in…

A: Chemical formula of Calsium acetate is (CH3COO)2Ca.

Q: ) Describe what happens when each of the following molecules is separately dissolved in water and…

A: An acid is a species which donates Proton while a base accepts proton.     an acid (A)after donating…

Q: An important component of blood is the buffer combination of bicarbonate ion and carbonic acid.…

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.