Given, pH of a solution Á is 3 and is mixed with another solution Bhaving pH 2. If both are mixed, then the resultant pH of the solution will be:

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

A: Given [NaCN]=0.459M [HCN]=0.269 PH =PKa+log( [NaCN] / [HCN] ) Ka= 6.2*10-10   ( from data ) PKa=…

Q: Which of the following is the most likely pH for a solution of calcium hydroxide and water?

A: The pH scale runs from 0-14. Neutral pH is 7.0.  The higher the pH (greater than 7) the more…

Q: 12.9 g of NaOH was dissolved in water affording a final volume of 250 mL. What is the pH of the…

A: Given :-  mass of NaOH = 12.9 g  volume of solution = 250 mL  To calculate :-  pH of solution

Q: Listeh A 250.00 mL sample of sulfuric-acid has a pH of 3.54. What is the value of for this solution?…

A:

Q: Calculate the pH of the following solution: 1.0 M H

A: pH = -log [H^+] Given -> [H^+]=1.0M

Q: A solution consisting of a strong acid with a concentration of 1721 millimoles has a volume of…

A: Number of moles =1721 millimoles  ...Or because, 1milli = 10-3    so,  = 1721 × 10-3 moles. = 1.721…

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

A:

Q: Calculate the pH of a solution that is 0.0330 M in

A: In all cases formula for weak acid to calculate pH is to be used. a. pH = 0.5pKa-0.5logC =…

Q: The pH of a solution is is 12.5. What are the hydronium ion and hydroxide ion concentrations in the…

A: At 25 degree Celsius.                                          PH + POH = 14.…

Q: If the ?b of a weak base is 5.8×10−6, what is the pH of a 0.33 M solution of this base?

A:

Q: the pH of a buffer solutiont

A:

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: Which of the following aqueous solutions are buffer solutions?

A: A buffer solution is an aqueous solution consisting of a mixture of a weak acid and its conjugate…

Q: The pH of a basic solution is 12.29. What is [OH]?

A: pH + pOH = 14

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: Without doing any calculations, which of the following acids, if in solutions of equal…

A: 11.  Ka is the ratio of  product of concentration of products raised to their stoichiometric…

Q: 10 mL of a strong acid solution with a pH of 2 is dilute to a volume of 100 mL. What is. the pH of…

A: The concentration of hydronium ion can be calculated from pH as shown below.

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0184 M solution. The pH of the…

A: Acids are the compounds which donate protons, H+ in the solution. Weak acids partially dissociate…

Q: When hydrogen ions are decreased, is the pH higher orlower?

A: The pH measurement is a scale to measure the nature (i.e., acidic or basic) of the solution. The red…

Q: A solution labeled 5 x 10M HCIO4 has a pH of. Do you see a problem with this answer? Briefly…

A: molarity is defined as  no.of moles of solute devided by volume of solution in liter. Whereas pH is…

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 0.355 M ammonium chloride and 7.65×10² M ammonia. The pH of this solution is

A: Mixture of Ammonium Chloride and Ammonia is a basic buffer solution. It's pH can be calculated by…

Q: A solution contains 0.252 M sodium nitrite and 0.179 M nitrous acid. The pH of this solution is

A:

Q: A solution is prepared by mixing 325 mL of 0.300 M NH3 and 325 mL of 0.300 M HCL. Assuming at the…

A:

Q: An aqueous solution contains 0.411 M Na,HPO4 and 0.436 M H,PO4. The pH of this solution is

A:

Q: A solution is made by titrating 7.00 mmol (millimoles) of HA and 3.00 mmol of the strong base. What…

A: Given, Ka(acid dissociation constant) of a weak acid = 5.61×10-6 A strong base is added to a weak…

Q: What is the use of the Nernst Equation to calculate pH in a solution?

A: ANSWER

Q: nobasic acids. pH value than CH,SO,OH with

A: An acid is a substance that gives H+ ions in its solution whereas a basic substance gives OH- ions…

Q: Aspirin, which is acetylsalicylic acid, was the first NSAID use to alleviate pain and fever. If a…

A: Since the concentration of H+ ions is always ( in any case) = concentration of H3O+  hence [H+] =…

Q: If the colour of a solution turns pink on adding few drops of phenolphthalein indicator, it means…

A: The colour of alkaline or basic solution turns pink on addition of few drops phenolphthalein…

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: Write ionization equations for a weak acid and its coniugate base. Show that adding these two…

A: Acids and bases can generally be classified under two categories, namely strong acids and bases and…

Q: A solution of three different weak acids is prepared and initially contains the following:

A:

Q: Calculate the pH and pOH of an aqueous solution that is 0.75 % HCI, by mass, and has a density of…

A: Given :-  % by mass of HCl = 0.75%  density of solution = 1.04 g/mL  To calculate :-  pH and pOH for…

Q: If the pH of a solution is increased from pH 5 to pH 7, it means that the

A: Given: pH of the solution is is increased from 5 to 7 To find: What will happen if above change…

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0180 M solution. The pH of the…

A:

Q: If pH of solution is 13, it means that if is:(a) Weakly acidic(b) Weakly basic(c) Strongly acidic(d)…

A: 1. To determine the acidity and basicity of the solution, the concept of pH was introduced. 2. pH…

Q: For a weak acid in solution (HA), how would adding a substance containing a common ion (A) affect…

A: When the solubility of a sparingly soluble compound decreases in presence of another compound having…

Q: What is the [H+], in moles per liter, in a solution with a pH of 2.500? Enter your answer to three…

A: pH is used to determine the concentration of hydronium ion. The expression of pH is shown below: pH…

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0194 M solution. The pH of the…

A: Given, a weak monoprotic acid is dissolved in enough amount of water to make the aqueous solution.…

Q: When 1x 10^-5 mole of NaOH is added to enough water to make 1 L of solution, the resulting solution…

A: First find the molarity and then pH.

Q: When in contact with a natural indicator, what color should the following substances be: (a) water,…

A: For Example, turmeric is a natural indicator and when it comes into contact with acid and neutral…

Q: The [?3?+] of a solution is 1.3 ? 10−5, Calculate the [??−], pH and pOH of the solution. Is the…

A: The concentration of H3O+ and the concentration of OH- in a solution are related to each other. The…

Q: What is pH of a solution consisting of 1.35 M NH3 and 2.08 M NH,NO,? K, of NH, is 5.8 x 10 10 0 9.13…

A: Given: Concentration of NH3 = 1.35 M Concentration of NH4NO3 = 2.08 M Ka for NH4+ = 5.8×10-10 We…

Q: Which one of the following 1.0 M solutions would have the highest pH?

A: A large Kb value indicates the high level of dissociation of a strong base. A lower pKb value…

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

A:

Q: A 0.0001 molar basic solution is 1.50 % ionized. What is the pH of the solution if its Kb= ?

A: pH of solution is defined by the number of H+ present in the solution.

Q: Which of the following cannot be used to measure the pH of a solution?

A: a] a . PH meter is used to measure the PH of a solution           where the hydrogen activity (…

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.