Calculate [OH−] for the following solution; [H3O+] = 8.87×10−9 M Is the solution basic at 25°C?

Q: [OH-] = 4.2 x 10-2 Express the concentration to two significant figures and include the appropriate…

A:

Q: Calculate either [H,O+] or [OH-] for each of the solutions at 25 °C. Solution A: [OH-] = 1.15 x 10-7…

A:

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: 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: Calculate either [H3O+] or [OH-] for each of the solutions at 25 °C. Solution A: [OH-] = 2.79 x 10-7…

A: The hydronium ion and hydroxide ion concentration are related to ionic product of water since they…

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: Calculate [OH-] for each of the following solutions, andindicate whether the solution is acidic,…

A:

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 3.8 × 10⁻⁴ M, then [OH⁻] is:

A: Given:         H3O+=3.8×10-4M         OH-=?

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

A:

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

A:

Q: Calculate either [H3O+] or [OH¯] for each of the solutions at 25 °C. Solution A: [OH-] = 1.57 × 10−7…

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: gaibrocat thoug wyr 2. Calculate the value of [OH-] from the given [H3O+] in each solution and label…

A: (H3O+) (OH-) = Kw =  1×10^-14

Q: What is the concentration of H3O+ ions in black coffee if [OH-] = 1.3 x 10-9 M? Is black coffee…

A:

Q: Calculate [H3O1] in a solution that has [OH-] = 6.7  M at 25 degrees celcius. Is the solution…

A:

Q: Calculate the [H+] and pH of a 0.0035 M nitrous acid solution. The ?a of nitrous acid is 7.10×10−4.…

A:

Q: Determine the [OH−] of a strong basic solution with a pH of 5.40 @ 25 degrees C.

A: Given, Temperature , T =25°C pH = 5.40

Q: 2. Complete the following tdde with the needed [H3O+], [CH], and pH, and dassify the solution as…

A:

Q: Calculate either [H,O*] or [OH-] for each of the solutions at 25 °C. Solution A: [OH) = 2.97 x 107…

A: Autoionization of water takes place as follows:In pure water, the concentration of hydronium ion and…

Q: [OH-] = 1.0 x 10-7 Express the concentration to two significant figures and include the appropriate…

A: Given-> [OH^-] = 1.0 × 10^-7 M   If [H3O^+] is 1.0 × 10^-7 M => then it is neutral .

Q: Calculate [H+] for each of the following solutions, andindicate whether the solution is acidic,…

A: pH = -log[H+] pOH = -log [OH-] pH + pOH = 14

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 6.7 × 10⁻⁴ M, then [OH⁻] is

A: In an aqueous solution [H₃O⁺] ×   [OH⁻]  = Kw

Q: Calculate [H+] for each of the following solutions, and indicate whether the solution is acidic,…

A: GIVEN :-  (a) [OH-]= 0.00045 M; (b) [OH-]= 8.8 X 10-9 M; (c) a solution in which [OH-] is 100 times…

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 2.4 × 10⁻⁴ M, then [OH⁻] is:

A: we have, [H3O+] =2.4 x10-4 M To calculate the concentration of OH-, firstly calculate the PH  of the…

Q: Calculate [H3O+] in a solution that has [OH-] =6.7 X 10-2 M at 25C. Is the solution neutral, acidic,…

A: For aqueous solution, the product of the concentration of hydronium and hydroxide ions is given by:…

Q: Calculate [H], [CIO], and [OH-] in an aqueous solution that is 0.110 M in HC1O4 (aq) at 25 °C. [H+]…

A: PH of the solution decides the solution is either basic or acidic ,if pH is less than 7 then…

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

A: pH +pOH = 14

Q: Calculate [H3O1] in a solution that has [OH-] = 6.7×102  M at 25℃. Is the solution neutral, acidic,…

A: Given,  concentration of the OH- ion = [OH-] = 6.7 × 102 M  Concentration of H3O+ ion = [H3O+] = ?…

Q: Calculate[OH-] if [H3O+] = 5.2 x 10-11M. Indicate whether the solutions is acidic, basic, or…

A: The term pH of the solution is a measure of the acidity or the basicity of a given solution. More…

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: If a solution has an [OH-]=1.2x10-3M and an [H3O+]=8.2x10-12M. Is the solution acidic, basic or…

A: The nature of the solution can be determined by calculating the pH of the solution. If pH >7:…

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 2.1 × 10⁻⁴ M, then [OH⁻] is

A:

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 7.5 × 10⁻⁴ M, then [OH⁻] i

A: For the acid-base reaction, a common solvent that is preferred is water. This is due to its…

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 8.6 × 10⁻⁴ M, then [OH⁻] is:

A: The question is based on the concept of PH and pOH calculations. pH is defined as negative…

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.