Calculate the pH of an NaOH solution where [OH-] = 4.6 x 10-5

Q: 3. Calculate the pH and pOH of 0.5 N solution of hydrochloric acid (HCI) at 25°C.

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Q: Calculate the pH of a 6.8 x 10-6 M solution of LiOH

A: Given: Concentration of hydroxide ion =

Q: Calculate 3OH-4 and pH for each of the following strong base solutions: (a) 0.182 M KOH

A:

Q: Calculate the pH of a solution if the concentration of H+ is 5.8 x10^(-6) M

A: pH = - log (H+) (H+)  = 5.8 × 10-6 M Substituting the concentration of hydrogen ion in above…

Q: What is the pH of a solution that has [OH-] = 6.0 × 10−12 M?

A: pH: pH is  justified  as power of hydrogen. pH=-log[H+] Or in general we can say that it helps us to…

Q: Calculate the pH of a 0.10 M HCOOH solution. Ka of HCOOH is 1.8 X 10-4.

A: pH is defined as the negative logarithm of hydrogen ion concentration present in the solution.…

Q: Calculate the pH of a solution with a hydrogen ion concentration of 4.5×10^-6 M.

A: Given that, in a solution, the hydrogen ion concentration is [H+] = 4.5×10-6 M. We have to calculate…

Q: Calculate the ph of the [OH-] = 2x10^-3 M.

A: We have to calculate the pH of given solution.

Q: If a solution has a [OH-] = 2.551 x 10-2 M, what is the pH of the solution?   Determine the [H3O+]…

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Q: Calculate the pH of a 2.4 x 10-5 M solution of LiOH.

A: Lithium hydroxide (LiOH) will dissociate to form hydroxide ions in a 1:1 ratio as per the equation…

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A: Dear student I have given answer to your question in the image format.

Q: Calculate [OH-] for a solution with a pOH of 8.03. What is the[H3O+] of this solution? What is the…

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Q: Calculate pH of 2.5 x 10-2 M NaOH(aq). NaOH(aq) is strong base.

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Q: What is the pH for a 0.05M solution of hydrochloric acid (HCI)? O -0.3 O 6.95 0.05 1.3

A: HCl is a strong monobasic protonic acid.

Q: Calculate the pH of a solution that has [OH-] = 5.9 x 10 -5 M

A: pH of any solution is given by  pH = 14 + log[OH- ]  where [OH- ] = concentration of OH- ions in the…

Q: 5. In a NaOH solution [OH2] is 2.9 x 10-24 M. Calculate the pH of the solution.

A: NaOH is  a strong base so, it completely dissociate into its ions in aqueous solution. NaOH (aq)…

Q: calculate the {H3O} of the solution of hydrochloric acid with pH = 2.00

A: Given, PH = 2.00 PH is defined as negative logarithm of concentration of [H+] ions.

Q: Calculate the pH of milk of magnesia whih has a [ OH- ] of 1.0 x 10-4 M.

A: [OH-] = 1.0 × 10-4 M  pH = ?

Q: calculate ph of 7*10^-3 M aqueous solution of Ca(OH)2 at 25 degrees

A:

Q: Calculate [OH-] for a solution where [H3O+]=0.00461 M. [OH-J= Calculate the hydronium ion…

A: Note: As per our guidelines, we are supposed to answer only one question. Please repost the other…

Q: Calculate the pOH and the pH of a 5.0 x 10^-2 M solution of NaOH.

A: Given :-A 5.0×10-2 M solution of NaOHwe have to calculate the POH and PH.

Q: Calculate the pH for an aqueous solution having a hydrogen ion concentration of 2.15 × 10-3 M.

A: pH = -log[H+] where [H+] = hydrogen ion concentration  Hence substituting the values we get  pH =…

Q: Calculate the pH, pOH, and [OH-1] of solution in which the [H3O+]=1.2x10-3

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Q: Show the calculation required to determine the pH of a solution that has H3O+ concentration of…

A: pH of solution is defined as negative logarithm of hydrogen ions.

Q: If the hydroxide concentration of a solution is [OH-] = 4.67 X 10-8 what would the pH of that…

A: Given:The concentration of OH, [OH-] = 4.67 X 10-8To find:pH = ?

Q: CALCULATE PH IF [H3O+] = 4.02 X 10 -3 AND [H3O+] = 8.99 X 10 -7

A: Given[H3O+] = 4.02 X 10-3 [H3O+] = 8.99 X 10-7pH = To be determined

Q: Determine the pH of an aqueous solution at 25.0 °C in which [H+] is 0.0025 M.

A: Given,     [H+] = 0.0025 M The pH of the solution is:

Q: Calculate [OH ]in an aqueous solution with a pH of 4.33 at 25°C. 6.3 x 10 6 O 3.8 x 10-5 O 2.1 x 10…

A: [19.]  pH = 4.33 (given)  [H+] = 10-pH  [H+] = 10-4.33  [H+] = 4.677 × 10-5 M Hence, [OH-] = 10-14 /…

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: What is the pH of 0.014 M solution of hydroiodic acid?

A: pH is a value that represents the concentration of hydrogen ions in solution. Hydrogen ions in…

Q: What is the pH of a solution that has [OH-] = 2.2 x 10-5 M?

A:

Q: Calculate the pH of 0.0250 M NaOH.

A: NaOH being a strong base easily dissociated into its respective ions in water. NaOH -------> Na+…

Q: a) Calculate [H3O+] when pOH is 8.90 b) Calculate the pH of an NaOH solution where [OH-] = 4.6 x 105…

A: Hello. Since multiple sub-parts of a question have been posted, the first three sub-parts shall be…

Q: If the [OH] of and acid is 2.57 x 10-8, what is the pH? o 13.2 o 12.49 ○ 6.41 o 2.91

A:

Q: Calculate the [H3O+] of a solution of hydrochloric acid with pH = 1.00 .

A: The relation between pH and [H3O+] is: pH=-log[H3O+]                        ...... (1)

Q: Calculate the concentration of an aqueous solution of NaOH that has a pH of 11.50.

A: • The values provided in the question are:-      i) pH of NaOH solution = 11.50    • We need to…

Q: Calculate the pH for 0.43 M NH4ClO4

A: pH can be calculated by following formula  pH = - log [H+]

Q: Calculate the pH of a 0.74 M solution of NaOH.

A:

Q: Find the pH of the following solution and state whether the solution is acidic, basic or neutral.…

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Q: Given [OH-]=5.2x10-6 M, Calculate its pH.

A:

Q: A solution has [OH-] = 8.9 x 10^-3, how would you calculate the ph of the solution ?

A: This problem can be solved by knowing that for any solution, pH + pOH = 14. The pH of a solution is…

Q: What is the pH of a solution that has [OH-] = 6.5 x 10-3 M?

A:

Q: Calculate the pH of solutions with the following concentrations. [OH−]= 1×10−12M

A: Given, [OH-] = 1 * 10-12 M   Required,                      pH of the solution   First, have to find…

Q: Calculate the pH of solutions having the following [H+]: (a) 0.0055 M (b) 1.54 x 10-8 M (c) 3.47…

A: The pH of any solution is given by, => pH = -log[H+ ]

Q: Determine the H*]. [OH , and pH of a solution with a pOH of 2.65 at 25 °C. (H = M %3D M pH =

A: Given data is as follows: The pOH of the solution = 2.65 As we know that; pH+pOH=14        At 25 °C…

Q: calculate the ph of [OH-]=8.7x10-6M

A: We have to calculate the pH of solution having given concentration.

Q: Calculate the pH of a solution with a H3O+ concentration of 5.8 × 10^-4 M

A: Given: Concentration of H3O+ = 5.8*10-4 M

Q: Calculate the pH of a solution with an H+1 concentration of 1.80 x10-2 M.

A: pH of any solution is given by  pH = -log[H+ ] where [H+ ] = concentration of H+ ions

Q: Calculate the pH and pOH of a 4.3 x 10-3M solution of NaOH.

A: Given information: Concentration of NaOH = 4.3 x 10-3M

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.