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

Q: Calculate the pH of a solution in which [OH−]=7.1×10−3M.

A: The pH of a given solution can be termed as a measure of its basicity or acidity. It is a measure of…

Q: Calculate the pH of a 0.008 M nitric acid (HNO3) solution.

A: We know that, HNO3 is a strong acid so completely dissociated. Thus, concentration of [H+]=0.008M

Q: The concentration of H3O+ in a sample of wine is 2.0 ×10-4 M. Calculate the pH of the wine.

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Q: Calculate the pH of a solution that has a hydronium ion concentration, [H3O+],[H3⁢O+], of 4.18×10−6…

A: The pH of the solution is = 5.38

Q: A chemist dissolves 724.mg of pure potassium hydroxide in enough water to make up 170.mL of…

A: potassium hydroxide will release hydroxide ions in the solution.

Q: Calculate the pH of an 0.025 M solution of HCl. HCl is a strong acid.

A: Concentration of HCl solution = 0.025 M   HCl is a strong acid. Therefore, HCl completely…

Q: Calculate the H+ ion concentration in a solution with a pH of 3.85.

A: Given values -> pH = 3.85

Q: The pH of a normal rainwater is 5.80. What will be the pH of rainwater that falls near a…

A: pH is negative logerathim of hydrogen ion concentration and is expressed by       pH = - log[H+]…

Q: The concentration of a strong base, X(OH)2 is 0.0321 M. What is the pH of this solution? 1.192…

A: Given The concentration of a strong base, X(OH)2 is 0.0321 M.

Q: What is the pH of a solution that has an OH- ion concentration of 3.20 M?

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Q: Complete the following table by calculating the missing entries. In each case indicate whether the…

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Q: Rainwater is found to be slightly acidic compared to pure water. It has a hydrogen concentration of…

A: Given: H+ of rainwater = 10-5.6

Q: Calculate the pH of a solution that has [H 3O +] = 5.2 × 10 –7 M.

A: pH is the potential of the hydrogen which is usually used to predict how strong an acid is. The pH…

Q: Enter your answer in the provided box. Calculate the pH of a 0.083 M Ba(OH)2 solution. pH =

A: The given base is strong base that dissociates completely into ions as,

Q: How does the hydronium ion concentration, (H3O+) change when the pH of a solution is lowered from…

A: pH = -log[H3O+]  log[H3O+] = -pH  so, [H3O+] = 10-pH

Q: Determine the pH of a 0.33 M solution of NH4Br

A: Since we know that, Pkb(NH3) = 4.74.. Since NH4Br is salt of strong acid and weak base..

Q: The normal pH range for human blood is 7.35 – 7.45. The patient’s blood has a concentration of…

A: Normal pH range for human blood =  7.35 – 7.45 [H3O+] = 8.91 x 10-8 M.

Q: Calculate the pH of an aqueous solution of 0.2100 M potassium carbonate. pH

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Q: Calculate the pH of each acid solution. Explain how the resulting pH values demonstrate that the pH…

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Q: Calculate the pH of a solution that has a hydroxide ion concentration, [OH−], of 8.95×10−7 M.

A: We have to calculate the pH of Solution.

Q: 2) Calculate the pH of a solution that has 1.3 x 106 M of aqueous H3O*. Is this solution acidic,…

A: The pH of an aqueous solution is determined by using the following equation-               pH=…

Q: Calculate the pH values of the following solutions. All solutions are prepared in water at 25 oC…

A: we have to calculate neutral pH of pure water at 40 °C

Q: Consider the following data on some weak acids and weak bases: name hydrofluoric acid acid acetic…

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Q: pH

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Q: The pH of a solution is a measure of the molar concentration of hydrogen ions, H* in moles per…

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

Q: Determine the pH of a solution that is 0.00542 M HCl and 0.0513 M HClO2. The Ka of HClO2 is 1.1 ×…

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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 hydroxide ion concentration, [OH−][OH−], for a solution with a pH of 3.15 What is the…

A: We know that, pH + pOH = 14 pH = - log[H+] pOH = - log[OH-]

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

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Q: Calculate the pH of an aqueous solution of 0.1930 M sodium carbonate. pH =

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Q: Calculate the pH of a solution that has a hydroxide ion concentration, [OH−][OH−], of 7.69×10−7 M.

A: Calculate the pOH of the solution,            pOH =- log [OH-]= - log (7.69 × 10-7)= 6.11

Q: Calculate the pH of a solution that has a hydronium ion concentration, [H3O+],[H3O+], of 5.79×10−5…

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Q: Determine the OH− in a solution with a pH of 3.7.

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Q: Calculate pH of 0.508 M solution of NaOH

A: By using the relation between pH and pOH we can solve this problem.

Q: Determine the pH of an aqueous solution where [OH] = 6.0 x 10 10 M.

A: Given data : [OH-] = 6.0 × 10-10 M.  To find : pH

Q: Acidity of a solution is determined by the concentration H of hydrogen ions in the solution…

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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.