Calculate the concentration of OH- in a 0.15 M solution of NH3.

Q: Calculate the [H3O+] for a solution in which [OH -] = 2.7 x 10-11 M. Is this solution acidic, basic,…

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Q: Determine the H+], OH-|, and pOH of a solution with a pH of 2.70 at 25 °C. [H*] = [OH] = РОН %3

A: Solution : pH       pH is a quantitative measure for the acidity or basicity of the solution. This…

Q: Find the [OH-] and pH of a 0.100 M NH3 solution.

A: It is given that the concentration of ammonia is 0.100 M.

Q: What is the pH of a 0.0257 M solution of NaOH (γγOH- = 0.889)?

A:

Q: What is the pH of a 0.087 M solution of HCl?

A: Given  [H+]     = 0.087 M  PH       =  ?

Q: Write an equation showing that rubidium hydroxide (RbOHRbOH) acts as an Arrhenius base in water.

A: Arrhenius base is defined as they give OH-in aqueous medium.

Q: What is the pH of a 0.00360 M solution of HCI?

A: Given, [HCl] = 0.00360 M PH is defined as negative logarithm of concentration of [H+] ions.

Q: Calculate the concentration of H3O* in a solution that contains 5.5 x 10° M OH" at 25°C. Identify…

A: • The values provided in the question are:-      i) Hydroxide ion concentration of a solution,…

Q: What is the pH of a strong acid (HA) of concentration 0.0135 M?   What is the pH of a strong base…

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Q: the concentration of OH- in a sample of seawater is 5.0 x 10-6 M. calculate the concentration of…

A: We have to predict the hydronium ion concentration.

Q: calculate ph of 0.15 M solution HCL at 25 degrees

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Q: Calculate the concentration of each species present in a 0.050-M solution of H2S.

A: Given,Concentration of H2S = 0.050 MH2S is a diprotic weak acid, therefore it will dissociate…

Q: Determine the [OH-], pH, and pOH of a 0.15 M ammonia solution

A: Construct ICE table and calculate the required values,

Q: If the hydronium ion (H3O+) concentration of a solution is 1 x 10-11 M (at 25°C), then what is the…

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Q: Explain why the hydronium ion, H3O-, is the strongest acid that can exist in aqueous solution. What…

A: In an aqueous solution, a strong acid exist as hydronium ion. The reaction equilibrium is given as,

Q: Calculate the hydroxide ion concentration, [OH−], for a solution with a pH of 8.52.         [OH−]= M

A: Given pH = 8.52  pH = - log [H+] 8.52 = - log [H+] log [H+] = - 8.52 = -9 + 0.48 log [H+] = log (…

Q: Find the [OH-] and pH of a 0.010 M Ba(OH)2 solution.

A: Given, 0.010 M Ba(OH)2

Q: Calculate the [H3O+] and pH of a 0.62M NaOH solution.

A: Given, Concentration of NaOH = 0.62M

Q: What are [H+] and [OH-] in a 0.00338 M solution of KOH

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

Q: Calculate the [H*], pH, and pOH in each of the following solutions in which the hydroxide ion…

A: The given question contains more than three sub-parts, so answer to first three sub-parts have been…

Q: (i) So?- + NH = HSO3 + NH3 (ii) HSO, + NH3 = Sož- + NH:

A: Given that,

Q: What is the pH of a solution with a concentration of 0.00001 moles/ml (M) of H1?

A: Gvien, concentration of 0.00001 moles/ml (M) of H1

Q: What is the pH of a 0.00645 M HCl solution?

A: pH can be calculated using the following formula. pH = - log [H+]

Q: Calculate the concentration of all species in a 0.500 M solution of H2SO3.

A:

Q: Given 1.5 M of NaOH, calculate the following: pH = POH = [H*] = M [OH] = M

A: NaOH is a strong base. So, pOH of NaOH can be expressed as -log [OH-] (where [OH-] = concentration…

Q: What is the pH of a .0832 M HCl solution?

A: Here given, Concentration of HCl = 0.0832 M, therefore-- [H+] = 0.0832 M We know, the formula--- PH…

Q: calculate the Ph of a 0.050M HCl solution

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Q: What is the pH of a 0.005 M aqueous HCl solution?

A: Given, concentration of HCl = 0.005 M HCl is a strong acid . It dissociates Completely in aqueous…

Q: What is the pH of a 0.00810 M solution of HCl?

A: pH of a Solution pH of a solution can be determined by the following formula pH = -log[H+ ] Where…

Q: Calculate the concentration of H3O+ and OH- in a sample of pH 3.30 solution?

A: As we know  pH = -log [H+] and pOH = -log[OH-]  and also pH+ pOH = 14

Q: Determine the pH of a 0.15 M solution of hydrabromic acid, HBr, at 25"C.

A: Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…

Q: What is the [OH-]  in a solution with a pH of 2.50?

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Q: Be sure to answer all parts. An aqueous solution of a strong base has a pH of 10.69 at 25°C.…

A: pH = 10.69  => pOH = 14 - pH = 14 - 10.69 = 3.31  [OH-] = 10-3.31 = 4.9 x 10-4

Q: What is the pH of an aqueous solution with an OH- concentration of 0.00250 M?

A: Solution:- Given concentration of OH- = 0.00250 M  [OH-] = 0.00250 M  As we know, p(OH) = -…

Q: Calculate the pH value of 0.5 M NaOH

A: As NaOH is very strong electrolyte i.e base so it will dissociate completely  :…

Q: NH3(aq) + H2O(l) ⇌ NH4+(aq) + OH-(aq) Identify the acid, base, conjugate acid, and conjugate base

A: A conjugate acid is formed when the base accepts hydrogen ions. Whereas, a conjugate base is formed…

Q: Given an OH- concentration of 0.10 M, calculate the H3O+ concentration, then identify the solution…

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Q: What is the relationship between H+ and OH- concentrations in a solution that has a pH of 11?

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Q: Which is the weak acid amongst the following ? NH4ОН, СН3СООН, НСІ, Ва(ОН)2 о кон O NH4OH NH4ОН NaOH…

A: An acid can be either strong or  weak according to the dissociation of the molecule in aqueous…

Q: What is the pH of (a) a 0.028 M solution of NaOH

A: Given: Concentration of NaOH=0.028M To find: The pH of the solution

Q: What is the ph of a 0.00130 M solution of NaOH

A: Concentration of NaOH = 0.00130 M  pH of the solution of NaOH = ?

Q: What is the pH of a 0.025 M solution of HCl?

A:

Q: What is the pH of a 0.00105 M solution of HCl?

A: HCl is a strong acid so it dissociates completely  in its aqueous solution.

Q: What is the concentration of H in 0.100 M hydrochloric acid, HCl?

A: Given that, Concentration of HCl solution = 0.100 M

Q: Calculate the concentration of H* ions in a 0.62 M NaOH solution.

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Q: Determine the concentration of OH- and H3O+ in a 0.0123 M solution of sodium cyanide, NaCN.

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Q: Calculate the pH of a 0.00015 M NaOH solution. NaOH is a strong base and completely dissociates in…

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Q: What is the pH of a 0.00760 M solution of NaOH?

A: Given concentration of NaOH = 0.0076 M

Q: The pH of 0.10M HNO3 is When a solution has pOH = 5.30, the [OH-] is

A: pH = -log[H+]  pOH = -log[OH-]

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.