When 25.0 mL of 0.400 M hydrobromic acid and 25.0 mL of 0.400 M potassium nitrite are combined, the pH of the resulting solution will be : A. Less than 7 B. Equal to 7 C. Greater than 7

Q: ph of 5% white vinegar is 2.22 Caculate the molarity. (5.00g acetic acid/ 100.00g solution) *asume…

A: Molarity is defined as “the mole of the solute per unit volume of the solution”. It is represented…

Q: Calculate the pH of the following solutions. a) 0.400 M HCl solution  b) Solution containing 0.727…

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Q: 14. Which indicator in yellow in a solution with a pH of 987 A methyl ornge R. hromthymol Mue C…

A: We have to tell which option is correct

Q: Calculate the pH of a mixture of 106 mL of 0.112 M HI and 30 mL  of 0.45 M KOH

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Q: The Ka of a monoprotic weak acid is 0.00258. What is the percent ionization of a 0.172 M solution of…

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Q: When 25.0 mL of 0.300 M hydrobromic acid and 25.0 mL of 0.300 M ammonia are combined, the pH of the…

A: pH of resulting solution will depend upon nature of resulting solution either acidic or basic.

Q: What is the final pH of a solution made by mixing 100 mL of 0.05 M CH3COOH and 100 ml of 0.1 M…

A: A buffer is a solution which resist any change in pH on adding a small amount of acid or base .   it…

Q: HF is a weak acid. If a solution of HF with a pH of 4.5 is made, Which of the following would be the…

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Q: 1 Determine the pH of the resulting solutions when the following reagents are mixed. a. 25.00mL of…

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Q: 10. Which of the following com JUSTIFY why. a. HCI and NaCl b. CH3COOH and KCH c. H₂S and NaHS

A:

Q: u make 50.00mL of a 0.045M solution of NaOH from a 2.5M stock solution. 9. How many milliliters of…

A: Answer: As, for the dilution, we add water in the solution, therefore moles of NaOH taken from stock…

Q: Calculate the pH of a mixture that contains 0.12 M of HCl and 0.20 M of HCH,O.

A: [HCl] = 0.12 M [H+] = 0.12 M [HC6H5O] = 0.2 M                              HC6H5O ⇔ C6H5O-  +  H+…

Q: what is the pH of a solution made by mixing 15.00 mL f 0.2M sodium hydroxide with 15.00 mL of 0.2M…

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Q: 8. A 1.000 L buffer solution contains 0.250 mol/L. NH, and 0.250 mol/L. NH, CL K=1.8x10 Determine…

A: We have to calculate the pH

Q: What mass of HCI should be used to make 175.0 ml of a solution with a pH of 2.80? The molar mass of…

A: Provided volume (V)=175ml Or, Provided volume (V)= 0.175litre Provided molar mass of HCl=36.46g/mol…

Q: Phosphorous acid, H3PO3(aq)), is a diprotic oxyacid that is an important compound in industry and…

A:

Q: What is the pH of a solution containing a mixture of 0.50 M HCN and 0.040 M NaCN? (Ka = 4.9 x 1010…

A: Answer :- HCN is a weak acid and NaCN is its conjugate Salt . This solution is basically acts as a…

Q: 28. How many grams of NaOH must be added to 0.30 L of water to make a 2.0% (w/v) solution? A) 60. g…

A: 28. Given :- volume of water = 0.30 L  % w/v = 2.0 %  To calculate :-  Mass of NaOH

Q: When 50 mL of 0.20 M ammonium nitrate and 50 mL of 0.10 M calcium hydroxide are combined, the pH of…

A: Volume of ammonium nitrate solution= 50 mL  Concentration of ammonium nitrate solution = 0.20 M…

Q: Suppose 0.5 L of 0.02 M HCI was mixed with 0.1 L of 0.1 M Ba(OH)2. Calculate the final pH of the…

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Q: A solution that contains a weak acid and its conjugate base in roughly equal concentrations is A.…

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Q: A solution is made by mixing 0.400M in formic acid, HCOOH, and 1.00M in sodium formate, HCOONa?…

A: Given -> Molarity of formic acid= 0.400 M Molarity of sodium formate = 1.00 M Ka = 1.80 × 10-4…

Q: 1. Which of the following is not a mixture? A jar filled with rocks and sand Sea water A cup of…

A: Concept is based on seperation of mixtures: As per our guidelines we have to answer first question…

Q: Calculate the pH of a solution prepared by mixing 150.0 mL of 0.200 M hydrobromic acid and 150.00 mL…

A: Applying concept of molarity and pH  pH = -log [H+]

Q: Calculate the after adding 10.00 mL of 0.15 M HCl to 50 mL of pure water b. Calculate the pH after…

A: for dilution  M1v1=M2V2  M1 =molarity before dilution V1=volume acid/base  M2 = molarity of solution…

Q: 6. A titration is carried out where 3.0 mL of 0.70 M NaOH is added to 15.0 mL of 0.150 M HCl. What…

A: Given, For NaOH solution Concentration of NaOH solution = 0.70 M = 0.70 mol/L Volume of NaOH…

Q: Calculate the pH of a solution that is made by mixing 50.0 mL of 0.15 M acetic acid and 50.0 mL of…

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Q: Calculate the pH of a solution containing 200ml of 0.01M Acetic acid and 80ml of 2.5M sodium acetate

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Q: A student dissolves a sample of a weak acid, HA, in 20.0 ml of H;O. The student then takes 5.6 mL of…

A: Given, Volume of water = 20.0 mL Volume of sample = 5.0 mL pH of final solution = 4.5

Q: 16. A 100.0 mL solution of 0.15 M acetic acid is tiated sing 0.20 M potassile hydroxide. Let's…

A: The objective of this question is to calculate the pH at the endpoint of a titration between acetic…

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.