1. Arrange the following liquids in order of increasing acidity. Wine, cow's milk, tomato juice, sea water, beer, lemon juice, drinking water, vinegar 2. Based on the auto-ionization of water, draw a graph showing the relationship of [OH-] and [H+]. Explain the relationship. 3. 5.00 g NaOH and 5.00 g Ba(OH)2 were used to prepare 1L solution each. Which solution will be more basic? (MM NaOH=40, Ba(OH)2=171.3) 4. 4.00 g KOH was added to the less basic solution in number 3. What will be the resulting pH of the solution? (MM KOH-56) a. You decide to test the pH of your brand-new swimming pool. The instruction manual advises to keep it between 7.2-7.6. Shockingly, you found out that the pH of your pool is 8.3! What kind of chemical should you add?

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 5.3 × 10⁻⁴ M, then [OH⁻] is:

A: Given [H3O+] = 5.3*10^-4 M  Kw = [ H3O+][OH-]

Q: Calculate the pH of a 0.094 M Ba(OH)2 solution. pH =

A: pH is determined by knowing the concentration of H+ ion in solution . Mathematically it is…

Q: + The pH of an acidic solution is 2.95. What is [H*]? 1 4 7 +/- 2 5 8 . M 3 6 9 0 C x 100

A: Given pH of acidic solution =2.95To find[H+]

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 1.4 × 10⁻⁴ M, then [OH⁻] is:

A: The concentration of OH- can be calculated as:

Q: + The pOH of an acidic solution is 9.47. What is [OH-]? 1 2 4 7 +/- 5 8 . M 3 6 9 0 冈 с x 100

A: The pOH of an acidic solution is 9.47. What is [OH] ?

Q: A solution has a pH = 8.57. Calculate the following: [OH-] = ___M pOH = ___ [H3O+] = ___M

A: The question is based on the calculations of PH and pOH. we have been given pH of the solution. we…

Q: Determine the [H+] in a solution with a pH of 4.39.

A:

Q: Calculate [ OH− ] for a solution where [H3O+]=0.00605 M .

A:

Q: If the pH of a solution is 1.78, what is the concentration of [H+]?

A: pH = -log [H+]

Q: 4. Complete the table. Classify each solution (each row) as acidic, neutral, or basic. [H*] [OH-] pH…

A:

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 2.3 × 10⁻⁴ M, then [OH⁻] is:

A: Here given---- [H3O+] = 2.3 ×10-4 M [OH-] = ? We know, dissociation of water occurs as---- H2O…

Q: Write the balanced NET IONIC equation for the reaction that occurs when ammonium chloride and sodium…

A: It is given that a reaction takes place when ammonium chloride reacts with sodium hydroxide.a) We…

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 7.6 × 10⁻⁴ M, then [OH⁻] is:

A:

Q: Complete the following table by calculating the missing entries. In each case indicate whether the…

A: we have to complete the given table

Q: concentration of OH

A:

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 1.2 × 10⁻⁴ M, then [OH⁻] is:

A:

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 1.3 × 10⁻⁴ M, then [OH⁻] is:

A: [OH-] = 7.7 x 10-11 M

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 6.3 × 10⁻⁴ M, then [OH⁻] is:

A: Using ionic product of water, concentration of hydroxyl ion can be determined from the hydronium ion…

Q: What is the hydronium ion concentration in an aqueous hydrobromic acid solution that has a pOH of…

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: Hydrogen selenide (H2Se) reacts with water according to the following equation. H2Se + H2O → SeH– +…

A:

Q: Classify the following as a strong acid or base or weak acid or base.

A: Strong acids are those which completely dissociate in aqueous solution  weak acids are partially…

Q: A solution contains mobile ions that conducts electrical current. Does the property describe a…

A: Movement of electric current through the metal wire is due to the electrons similarly the…

Q: For a solution of 0.15 M HF, the [H+]  0.15 M.  Why?  What is the [H+]?  What is the pH of the…

A:

Q: Write an equation for the reaction that takes place when each acid is added to water. For a…

A: When acid is added into water then ionisation of acid take place.

Q: the [H^+] of a solution is 2.5 x 10^-4M, what is the concentration of the hydroxide ion ? __ Is this…

A:

Q: pH = 6.35

A:

Q: What is [H+] concentration if pH=0?

A: pH is a scale to measure the concentration of hydrogen ions. The negative logarithm of hydrogen ion…

Q: An aqueous solution at 25°C contains [H3O+] = 4.90 x 10-3 M. The pH of the solution is calculated by…

A: The concentration of hydronium ions is .The temperature given is .To find the value of the pH of the…

Q: Calculate [H3O+] and [OH−] for each of the following solutions at 25 ∘C given the pH. pH= 11.31

A:

Q: In an aqueous solution at 25 °C, if [H₃O⁺] = 7.2 × 10⁻⁴ M, then [OH⁻] is

A: Given,[ H3 ] = 7.2 x 10-4 M at 25.0 oC

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 1.1 × 10⁻⁴ M, then [OH⁻] is:

A: We know that  Kw  for water  =  10-14 at 25oC Given [H3O+] concentration is 1.1×10-4 M      [ OH-] =…

Q: A) An aqueous solution has a hydrogen ion concentration of 1.0 x 10^-13 M. What is the hydroxide…

A: For an aqueous solution, we know that the production of the concentration of the hydrogen ions and…

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.