Question 18:Calculate the [H3O+] value of each aqueous solution. Part A: NaOH with [OH−]=1.6×10−2M Part B: aspirin with [OH−]=2.8×10−11M. Part C: seawater with [OH−]=3.0×10−6M

Q: What is the [H3O+] of a solution if [OH−] is 5.0 × 10−8 M?

A:

Q: Assuming complete dissociation, what is the pH of a 4.15 mg/L Ba(OH)₂ solution? pH =

A: Upon dissociation the base will give the hydroxide ions which will make the solution basic and from…

Q: Enter your answer in the provided box. If the OH−ion concentration of a blood sample is 6.1×10−7 M,…

A: pOH of the blood sample is calculated,

Q: For each of the following strong base solutions, determine [OH−],[H3O+][OH−],[H3O+], pHpH, and…

A: The objective of the question is to determine the concentration of hydroxide ions [OH-], hydronium…

Q: Determine the concentration of H+H+ ions in an aqueous solution where [OH−]=1.45×10−4…

A: Given: [OH−]=1.45×10-4 M [H+] =?

Q: Calculate [OH-] given [H3O+] in the aqueous solution. [H3O+]=3.3*10^-3 M

A: pH of the solution is given by,                               By using given concentration to get…

Q: Fill in the pH value (with 2 decimal places) for each solution listed 0.10 M HBr: 0.25 M HCI:…

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

Q: An orange juice has a pH of 3.30. Calculate its [OH-] and [H+].

A:

Q: For 8.73 x 10-3 M LiOH, determine [OH-] and [H3O+]. Express your answers in moles per liter to three…

A: Lithium hydroxide is a strong electrolyte and it dossociates completely as follows:Hence the…

Q: For a given aqueous solution, if [OH-]=1.0x10^-12 M what is [H+]

A: For the aqueous solution, the concentration of the hydrogen ion and hydroxide ion is constant at a…

Q: Calculate the  [H3O+]  value of each aqueous solution. NaOH  with  [OH−]=1.4×10−2M  Express your…

A: We know the relations ;  pH = -log[H3O+]  And ,pOH = -log[OH-] And , pH + pOH = 14

Q: What is the [ H3O+] in a solution that has a [OH-] = 9.0×10−2 M?

A: Given, Concentration of OH- = 9.0 * 10-2 Concentration of H3O+ =? By using the autoionization…

Q: Calculate the OH- ion concentration of a 6.2 x 10^-3 M HClO3 solution

A:

Q: Calculate [OH−][OH−] given [H3O+][H3O+] in each aqueous solution [H3O+]=6.2×10^−4M?

A: Here we have concentration of  i.e. [H3O+]=6.2×10^−4M From this we can calculate pH first pH = - log…

Q: How many ml of 0.250 M HCl are required to completely neutralize 75.0 ml of 0.600 M Ba(OH)2…

A: For the complete neutralization: Number of miliequivalents of acid  = Number of miliequivalents of…

Q: concentration of OH

A:

Q: if the concentration of OH- in an aqueous solution is 1.4 x10^-7 M, the concentration of H3O+ is…

A: Given;

Q: Determine [OH−] of a solution that is 0.290 M in HCO3− . ( Ka1 for H2CO3 is 4.3×10−7 .)

A: For the given weak acid , dissociation constant Ka = 4.3 * 10-7First we have to calculate the H+…

Q: for a given aqueous solution if [OH-]=7.11x10^-10 M what is [H+]

A: For the aqueous solution, the product concentration of the hydrogen ion and hydroxide ion is…

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 [H+] concentration in a solution with a pH of 4.9

A: The pH is defined as the negative log to base 10 of concentration of hydronium ion. The Hydronium…

Q: Determine [OH−][OH−] of a solution that is 0.220  in HCO3−HCO3−. (Ka1 for H2CO3H2CO3 is…

A: Given,molarity of HCO3- = 0.220 MKa1 of H2CO3 = 4.3 x 10-7H2CO3 (aq) + H2O (l)    HCO3- (aq) + H3O+…

Q: 9) Calculate [H] in each aqueous solution at 25°C & classify solution as neutral, acidic or basic.…

A: Answer:- The solution which has higher hydrogen ion concentration than that of hydroxide ion…

Q: The OH- concentration in an aqueous solution at 25 celcius  is 7.1 x 10^-5. what is [H+]?

A: Given,  Concentration of OH-ion = [OH-] = 7.1 x 10-5 M  What is [H+] = ?

Q: Calculate [OH-] given [H3O+] in the aqueous solution. [H3O+]= 7.1 * 10^-9 M

A: Given information: Concentration of H3O+ = 7.1×10-9 M

Q: Tell the concentration and if it’s an acid or base 1. [OH-]=5.48 X 10 ^-9 M 2.[OH-]=2.0 X 10^-13 M

A:

Q: A new drug obtained from a plant was found to be a weak organic base. A solution of this weak base…

A:

Q: Calculate [OH−][OH−] given [H3O+][H3O+] in each aqueous solution [H3O+]=5.6×10^−12M

A:

Q: Calculate [OH-] given [H3O+] = 4.0 * 10^-9 M

A: An acidic substance is the substance that can give H+ ions. They are corrosive and sour in nature.…

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

A:

Q: Calculate [OH-] given [H3O+] in the aqueous solution. [H3O+]= 8.2 * 10^-4 M

A: pH of the solution is given by,                     By using given concentration to get the pH of…

Q: What is the concentration of OH^- in a solution with a pH of 10.00

A: The objective of this question is to find the concentration of hydroxide ions (OH-) in a solution…

Q: At 25°C, what is the hydroxide ion concentration, [OH−], in an aqueous solution with a hydrogen ion…

A:

Q: Assuming complete dissociation, what is the pH of a 4.04 mg/L Ba(OH)2 solution? pH=

A: Given :  We have to calculate pH.

Q: What is the [H+] when a PH is measured at 7.8?

A: Given that : The pH of the solution = 7.8 We have to calculate the concentration of H+ ions in the…

Q: What is the pH of a solution with [H+] = 3.51x10-5 M

A:

Q: What is the pH of a solution if the [H+] = 7.2 x 10^-9?

A: The pH is a scale that is widely used to measure the acidity or basicity of a solution. The pH is…

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 6.2 × 10⁻⁴ M, then [OH⁻] is:

A: pH +pOH = 14

Q: The concentration of H+ in a solution is 1×10−2 M. What is the hydroxide ion concentration?

A: The objective of this question is to find the concentration of hydroxide ions (OH-) in a solution…

Q: Assuming complete dissociation, what is the pH of a 4.12 mg/L Ba(OH)₂ solution? pH =

A:

Q: graph

A: At Volume of NaOH = 0.0mL then, pH = 3.1  pH = -log[H+]  [H+] = 10^-pH  [H+] = 10^-3.1  [H+] =…

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.