2. 30 mL of a 0.4375 M HCI solution are added to 35 mL of 0.250 NAOH solution. What is the final pH?

Q: The pH of a basic solution is 12.03. What is [H⁺]?

A: Given: pH of solution = 12.03

Q: A solution contains 0.377 M potassium acetate and 8.75×10² M acetic acid. The pH of this solution is

A: Given :-  concentration of potassium acetate = 0.377 M  concentration of acetic acid = 8.75 × 10-2 M…

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: The pH of a solution that contains 0.010 M H3O+ is

A: The concentration of [H3O+] = [H+] = 0.01 M.

Q: 50 mL of 0.02 M NaOH is added to 25 mL of 0.04 M HCl solution. The pH of the resulting solution will…

A: Balanced chemical equation: NaOH (aq)  +   HCl (aq)   ------->  NaCl (aq)  +  H2O (l) Number of…

Q: The pH of an acidic solution is 2.19. What is [OH]?

A: The question is best on the concepts of PH. we have to calculate hydroxide Ion concentration.

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: Is it possible for a solution to have a negative pH? If so, would that pH signify a basic or acidic…

A:

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

A:

Q: Consider two solutions, solution A and solution B. 3H+4 in solution A is 250 times greater than that…

A: A solution has pHA  = - log [HA +]  and [HA +] is the concentration of Hydrogen in solution A . B…

Q: A solution contains 0.392 M NH¸I and 0.134 M ammonia. The pH of this solution is

A:

Q: The pH of an acidic solution is 6.53. What is pOH?

A: We know that  pH + pOH = 14

Q: 30 ml of a 0.4375 M HCl solution are added to 35 ml of 0.250 NaOH solution. What is the final pH ?

A: given :-  molarity of HCl solution = 0.4375 M  volume of HCl solution = 30 mL  molarity of NaOH…

Q: A solution is made by dissolving 22.3 g of HONH₃ClO₃ in 500.0 mL of water. Using Ka(HONH₃⁺) = 9.1 ×…

A: OHNH3ClO3 dissociates to give H+ ions in the solution. The net ionic equation is:

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

A:

Q: A solution of sodium acetate (NaCH3COO0 has a pH of9.70. What is the molarity of the solution?

A:

Q: Suppose that 250.0mL of a basic solution is 0.100 M in KOH. What volume of a 0.200-M HCL solution…

A: Given: The neutralization reaction of KOH is as follows, The moles of hydroxide ions are…

Q: Determine molarity of NaOH solution based on pH. pH of NaOH is 13.27

A: The number of moles of a substance is given as the mass of the substance upon its molar mass. The…

Q: What is the pH and how is it calulated when 100 ml of 14% acetic acid is added to 200 ml of water.

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: 5.07 g of HCl(g) is dissolved in water to make a 220 mL solution. Calculate the pH of the solution.

A: Since you have posted multiple questions we are answering first question for remaining question to…

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: The pH of an acidic solution is 2.79. What is pOH?

A: pH of a solution is a measure of hydronium ion concentration [H3O+] or hydrogen ion[H+] in the…

Q: A) A 1000.0 mL sample of lake water is titrated using 100 mL of a 0.100 mol/L base solution. What is…

A: Given: Volume of lake water (V1) is 1000.0 mL. Molarity of base (M2) is 0.100 mol/L. Volume of base…

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: A solution contains 0.119 M sodium cyanide and 7.32×10-2 M hydrocyanic acid. The pH of this…

A:

Q: The ph of 168 mL of a .556 M solution of unknown weak base is 12.96. what is the Kb of this base?

A: Volume of solution =168 mL Concentration of solution=0.556 M pH =12.96 Kb=?

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

A:

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

A: Ph= -log [H+] [H+]= 10-14÷[OH-] Lowest PH=C5H5N  (1) For C5H5NOH- = k6xC = 1.7 x 10-9x1…

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

A:

Q: A solution contains 8.64x102 M potassium nitrite and 0.370 M nitrous acid. The pH of this solution…

A:

Q: The pH of an acidic solution is 4.17. What is pOH?

A: pH and POH is defined for acid and base. We have relation between them so we will use the same

Q: A solution contains 0.129 M ammonium chloride and 7.45x102 M ammonia. The pH of this solution is

A: Given :-  [NH4Cl] = 0.129 M  [NH3] = 7.45 × 10-2 M  To calculate :  pH of solution

Q: An aqueous solution contains 0.372 M KHS and 0.361 M H,S. The pH of this solution is

A: As per our guidelines, we are supposed to answer?️ only one question. Kindly repost other questions…

Q: A solution contains 0.207 M sodium nitrite and 9.30×10-2 M nitrous acid. The pH of this solution…

A: Given, concentration of sodium nitrite, [NaNO2] = 0.207 M            concentration of nitrous acid,…

Q: What is the pH of the final solution?

A: In order to calculate the pH we first write down the given data: Volume of salt=28.5ml=0.0285L.…

Q: The pH of an acidic solution is 6.75. What is pOH?

A:

Q: The pH of a basic solution is 12.51. What is pOH?

A:

Q: What volume of a concentrated HCl solution, which is 36.0% HCl by mass and has a density of 1.179…

A: Given : Percent by mass of HCl = 36.0 % Density of solution = 1.179 g/mL Volume of HCl solution to…

Q: A solution contains 0.342 M sodium acetate and 0.112 M acetic acid. The pH of this solution is .

A:

Q: 3) Identify two salts that will dissolve to give (a) an acidic solution, (b) a basic solution, and…

A: (a) Acidic solution - Copper sulphate (CuSO4)  and Ammonium chloride (NH4Cl)  (b) Basic solution-…

Q: The pH of a basic solution is 12.89. What is [H⁺]?

A:

Q: Suppose that 250.0 mL of a basic solution is 0.100 M in KOH. What volume of a 0.200-M HCl solution…

A:

Q: A solution is made by dissolving 27.5 g of HONH₃ClO₃ in 500.0 mL of water. Determine the pH of the…

A: Given: Mass of HONH₃ClO₃ = 27.5 g Volume of Water = 500.0 mL To Calculate: The pH of the solution

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

A:

Q: The pH of a basic Solution is 10.27 what is [H+]?

A: At, 25°C, ionic product of water, Kw is given by: Kw = H+OH- = 10-14 Now, pH and pOH is given by: pH…

Q: Sorry for the incomplete question. Here is the complete one: Determine the pH of a single solution…

A: Acid is a compound which gives hydrogen ions in solution and base gives hydroxide ion in solution.

Q: Calculate the pH of each of the following strong acid solution 0.225 g of HClO3 in 2.00 L of…

A: Given data contains, Mass of HClO3 is 0.225 g. Volume of the solution is 2.00L. The moles of HClO3…

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.