determine the pH of a 0.0006 M NaOH solution

Q: Calculate the PH of a 0.012 M solution of HCl

A: pH is used to determine the concentration of hydronium ion.

Q: Calculate the pH of the following solution: 50 M HNO3

A:

Q: Calculate the pH of the following solutions. 5.00 g of HBr in 100 mL of the aqueous solution

A: Given, mass of HBr = 5.00 g            volume of HBr = 100 mL Now, let us calculate the moles of…

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

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

Q: The pH of a solution of 0.200 M NaOH is __________.

A: • The values provided in the question are:-     i) Concentration of sodium hydroxide solution,…

Q: Determine the pH of the following: a single solution prepared to final concentrations of 0.01469 M…

A: pH is the negative logarithm of hydrogen ion concentration. When an acid is mixed with a base, both…

Q: Find the pH of a 0.010 M HNO2 solution.

A: HNO2 is a weak acid with dissociation constant, Ka = 7.2 X 10-4  Hence HNO2 will dissociate…

Q: Calculate the pH and the concentrations of all species in a 0.1500 M NH4NO3 solution.

A:

Q: Determine the pH of the following solutions, using the information provided. 1.25 ×10–3 M HNO3…

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Q: What is the pH of a 0.00100 M solution of NaOH?

A: Inorganic chemistry.

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

A:

Q: Calculate the pH of a  0.500 M HCN solution.

A:

Q: A solution of sulfuric acid (H2SO4) has a concentration of 0.0075 M. Calculate the pH of this…

A: Given, Concentration of H2SO4 solution = [H2SO4] =  0.0075 M pH of the solution = ? Note:  Sulfuric…

Q: Calculate the concentration of all species present and the pH of a 0.020-M HF Solution.

A: Concentration of HF = 0.020 MKa(HF) = 3.5 * 10-4Chemical reaction of HF in water Chemical Equation…

Q: Calculate the pH of a 0.015 M solution HBr .

A: Strong acid:The solution that is completely dissociates into its ions in water. This makes to…

Q: Determine the pH of a 0.0020M barium hydroxide solution.

A:

Q: Determine the pH in a 0.235 M NaOH solution.

A: pH can be calculated using pOH.

Q: Determine the pH of an HNO, solution of each concentration. In which cases can you not make the…

A: a) To determine the pH of 0.500 M HNO2 and if the assumption is valid or not, HNO2 + H2O ⇌NO2-+…

Q: Calculate the pH of 0.024 M chloric acid

A:

Q: pH

A:

Q: Calculate pH of a solution that has hydrogen ion (H+) concentration of 0.044 M

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Q: what is the ph of a solution whose hydrogen ion concentration is 0.015?

A: As we know, HCl is a stong acid. It dissociates completely into H+ and Cl—in a chemical equation –

Q: Calculate the pH value of 0.5 M NaCl

A: There can be 4 type of combinations of salt:A salt formed when a strong acid combines with a strong…

Q: Find the pH of a 0.0025 M HCl solution.

A: Here we are required to find the pH of 0.0025M of HCl solution

Q: The pH of an aqueous solution of 0.549 M hydrocyar

A: HCN is a weak acid , weak acid does not dissociate completely hence it's pH can be calculated as…

Q: Calculate the pH of a solution that is 0.142 M HCL?

A:

Q: Enter your answer in the provided box. Calculate the pH of a 0.0825 M HCl solution. pH =

A: HCl completely dissociates since it is strong acid.The concentration of H+ ions for a 0.0825 M HCl…

Q: Determine the pH of the following: 1. 0.02850 M µM Mg(OH)2

A: [OH]- = 2 × [Mg(OH)2] + 10-7 M = 2 × 0.02850 × 10-6 + 10-7 M = 1.57 × 10-7 M

Q: calculate the Ph of a 0.050M HCl solution

A:

Q: Find the pH of a 0.043 M HClO4 solution.

A: Given :- concentration of HClO4 = 0.043 M  To calculate :- pH of the solution

Q: Consider a solution which is [OH-] = 1.0 x 10-5 M. Calculate the pH of the solution. Calculate the…

A: Applying formula [H+][OH-] = 1×10-14 And PH = -log[H3O+]

Q: Calculate the pH of a 0.27 M sodium carbonate solution. pH= i

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Q: Calculate the percent ionization of a 0.489 M solution of hypochlorous acid. % Ionization =

A:

Q: Calculate the pOH and pH of a 0.0045 M solution of NaOH.

A: concentration of NaOH solution is 0.0045 M  we have to find pH and pOH of solution  pH = -log[H+]…

Q: Calculate the pH of 0.71 M Ca(OH)2 solution. Provide your answer to two places after the decimal and…

A: Given :- molar concentration of Ca(OH)2 solution = 0.71 M  To calculate :- pH of solution

Q: Determine the pH of a 1.00×10¯7 M aqueous solution of HBr.

A: Given : concentration of HBr solution = 1.00 × 10-7 M  To calculate :- pH of solution

Q: The pH of a 0.0037 M solution of HNO₃ is

A:

Q: Calculate the pH of the solution.  Assume 1.0 L of solution. You must identify the type of solution…

A:

Q: Define pH of a solution. Calculate the pH of a 1.37M solution of HCI.

A: pH is the negative logarithm of concentration of H+ ions  pOH is the negative logarithm of…

Q: Calculate the pH of a solution with a hydrogen ion concentration of 0.0003 M

A: Given  concentration of hydrogen ion = 0.0003 M We have to calculate the pH of solution.

Q: Calculate the pH of a 0.052

A: Since the LiOH is a strong base, it completely dissociate into ions in its solution. So the…

Q: calculate the ph of a 0.000427 M barium hydroxide solution.

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Q: Calculate the pH of a 0.55 M solution.

A:

Q: Obtain the pH corresponding to the following hydronium-ion concentrations. 6.35 x 10-9 M

A:

Q: Calculate the pH of the following acid or base: 2. 2.0x10 M NaOH

A: Given: [NaOH] = 2.0 x 10-4 M = [OH-] pOH = - log[OH-]          = - log (2.0 x 10-4 )         = 4 -…

Q: Calculate the pH of a solution if [H*] is measured to be 5.76 x10-9 M. Is this solution acidic or…

A: Given: Concentration of [H+] ion = 5.76×10-9 M

Q: Calculate the pH of a solution that has [H3O+] = 3.9 × 10−8 M.

A: We are given  [H3O+]  = [H+] = 3.9 × 10−8 M we are to calculate the pH.

Q: Calculate the pH of a 0.00118 M solution of HBr.

A: Given data contains, Concentration of HBr is 0.00118 M. Hydrobromic acid is a strong acid so it gets…

Q: Calculate the pH of the following solutions 0.0040 M Ba(OH)2

A:

Q: If the pH of a solution is 9.7, calculate [H*]. O 70794.578438414 O 5011872336.272714615 O…

A: pH = - Log[H+] [H+]= -antilog[pH] [H+]= antilog[-9.7] [H+] = 1.99 * 10-10

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.