if 50 mL of .5 M NaOH is added with 30 mL of .5 M HCL, what will be the pH of the solution

Q: if 0.1L of 0.2 HCL is added to 0.9 L of water what is the resultant pH?

A:

Q: A solution contains 0.119 M ammonium chloride and 0.126 M ammonia. The pH of this solution is

A: The given data contains, Molarity of ammonium chloride = 0.119 M. Molarity of ammonia = 0.126 M pKb…

Q: 20.0 ml of 0.01 M HCl is added to    5. 6    ml  0. 10 M NaOH, the resulting pH of the solution will…

A:

Q: Calculate the pH of the resulting solution when 20.0 ml of 0.25 M HCl is added with 20.1 ml of 0,25…

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

Q: A solution contains 0.437 M sodium acetate and 0.397 M acetic acid. The pH of this solution is

A: Given : concentration of sodium acetate = 0.437 M  Concentration of acetic acid = 0.397 M  To…

Q: A solution contains 0.459 M sodium cyanide and 0.269 M hydrocyanic acid. The pH of this solution is

A: In buffer solution  salt and acid concentration given than ph eaisly calculated.

Q: Which theory or concept can explain buffer solution precisely? Explain your answer.

A: a buffer solution is formed by mixture of weak acid and its conjugate base or weak base and its…

Q: A solution contains 0.408 M sodium acetate and 0.145 M acetic acid. The pH of this solution is

A:

Q: A solution contains 0.160 M sodium cyanide and 0.255 M hydrocyanic acid. The pH of this solution is

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Q: A 15 ml solution is 0.50 HCI. If 0.2 M NaoH is to added to this solution Calculate the pH of…

A: Given, Volume of HCl solution = 15 mL Concentration of HCl solution = 0.50  Concentration of NaOH…

Q: A solution contains 0.131 M sodium cyanide and 0.359 Mhydrocyanic acid. The pH of this solution is

A:

Q: If 5.00 mL of 6.00M HCl is added to 95.00 mL of purewater, the final volume of the solution is…

A: If 5.00 mL of 6.00M HCl is added to 95.00 mL of pure water, the final volume of the solution is…

Q: A solution contains 0.297 M ammonium chloride and 0.246 M ammonia. The pH of this solution is

A:

Q: A solution contains 0.420 M CH3NH3 and 0.143 M methylamine, CH3NH2. The pH of this solution is .

A: Given : Concentration of CH3NH3+ = 0.420 M And concentration of CH3NH2 = 0.143 M Since the solution…

Q: If 5.00 mL of 0.500 M NaOH are added to 10.00 mL of 0.300 M HCl, what is the final pH?

A: pH is used to measure the concentration of hydronium ion.  The expression for the calculation of pH…

Q: A solution contains 0.171 M ammonium iodide and 0.339 M ammonia. The pH of this solution is

A:

Q: In titration of 50 ml of 0.1 M NaOH solution with 0.2 M HCl, which is the pH after adding 30 ml of…

A: For the given titration the volume of NaOH solution is 50 mL and the molarity of the NaOH solution…

Q: 0.0155L of a 0.505M solution of HCl is combined with 0.0482L of a 0.0175M solution of NaOH. What is…

A:

Q: The pH of a solution that contains 1.2M acetic acid and 0.920M sodium acetate is?

A: pH of weak acid = 4.63.

Q: A solution contains 0.219 M potassium nitrite and 0.218 M nitrous acid. The pH of this solution is

A:

Q: A solution contains 0.145 M ammonium chloride and 0.108 M ammonia. The pH of this solution is

A:

Q: 0.1M acetic acid is in a buffered solution with sodium acetate. the ph is 5.50 what is the…

A:

Q: Which things should be considered while deciding weak acid/conjugate base pair to make a buffer…

A: Buffer solution: The buffer solution is an aqueous solution consisting of a mixture of a weak acid…

Q: If 990. mL of water is added to 10.0 mL of 0.10 M HCl, what is the pH of the resultant solution?

A: Given that,  Volume of water = 990 mL Volume of 0.10 M HCl = 10.0 mL When volume of water and HCl…

Q: To a 50 mL of 0.1 M HCL solution, 10 mL of 0.1 M NaOH is added and the resulting solution is diluted…

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Q: Enough of a monoprotic acid is dissolved in water to produce a 1.11 M solution. The pH of the…

A: The concentration H3O+ of weak acid [H3O+] = Ka*C  where Ka is the dissociation constant, C is the…

Q: A buffer solution is prepared by combining 0.898 moles of formic acid and 0.733 moles of sodium…

A: The buffer solution is prepared by mixing with 0.898 moles of formic acid and 0.733 moles of sodium…

Q: A solution contains 0.280 M ammonium iodide and 0.161 M ammonia. The pH of this solution is

A: Given: Ammonium iodide [NH4I]= 0.280 M Ammonia [NH3] = 0.161 M pH = ? The given solution is a buffer…

Q: A student adds universal indicator to a solution. The color is found to be light orange. What is the…

A: The universal indicator is a pH scale very vibrantly divided into different colors. Ph range is from…

Q: A solution was prepared by mixing 50.0 mL of 0.10 M HCl and 25.0 mL of 0.25 M NaOH. What is the pH…

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Q: A solution contains 0.251 M potassium cyanide and 0.454 M hydrocyanic acid. The pH of this solution…

A:

Q: Calculate the pH of the resting solution when 100mL of soln A has 50 mL of soln C added to it

A:

Q: Suppose 90.00 ml of 0.200M HCI is added to an acetate buffer prepared by dissolving 0.100 mol of…

A: Volume of HCl = 90.00 mLConcentration of HCl = 0.200 MNumber of moles of acetic acid = 0.100…

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.