A solution containing 572.0mL of 0.6300MHCl is diluted to a volume of 1.000L. What is the pH of this solution?

Q: A solution is made by dissolving 0.02500 moles of Ba(OH)2 in enough water to make 750. ml of…

A:

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: A solution is prepared by diluting 0.55 mol HNO3 with water to a volume of 1.75L. What is the pH of…

A: Molarity = Number of moles of solute/Volume of solution in L pH = -log[H+]

Q: A sample of 1.25 L of HCl gas at 21 °C and 0.950 atm is bubbled through 0.500 L of 0.150 M NH3…

A: According to ideal gas law (for HCl moles calculation), PV = nRT where P = pressure = 0.950 atm V =…

Q: A sample of vinegar contains 40.0 g of acetic acid (CH3COOH) per liter of solution. Suppose 1.00 mL…

A: The molecular weight of acetic acid is 60.05 g/mol. 40 g of acetic acid is present in 1 L of…

Q: A solution is made by dissolving 0.06100 moles of Ba(OH)2 in enough water to make 250.0 mL of…

A: Given, moles of Ba(OH)2 = 0.06100 moles Volume of the solution = 250.0 mL = 0.250 L pH of the…

Q: A solution of HA, a weak acid (K = 0.0040), is prepared with a concentration of 0.579 M. Determine…

A: Given Data :  1. Ka =0.0040  2. Concentration of HA = 0.579 M

Q: A solution is prepared by adding NaOH to pure water until a pH = 9.34 is obtained. Calculate the pH…

A:

Q: A solution is prepared by diluting 20.0 mL of 0.0010 M HCl to a final volume of 2.00 liters. What…

A: Consider the given information is as follows; Volume of initial HCl solution V1= 20.0 mL = 0.02 L…

Q: Calculate the pH of a solution containing 0.10 mol/L ammonia, NH,. Kb for ammonia is 1.8x10-.

A: The concentration of ammonia = 0.10 mol/L = 0.10 M (mol/L = M) Kb for ammonia, NH3 = 1.8×10−5

Q: Calculate the pH of the solution that is 0.0300M carbon dioxide. (validate your…

A: pH: pH value can be generally used in the identification of charector of specific solution (acidic…

Q: Suppose 0.100 mol of NaCH3COO is dissolved in enough water to make 1.00 L of solution. What is the…

A: pH is referred to the potential of hydronium ion and is calculated by taking the negative log value…

Q: if 65ml of 0.25M naoh are combined with 76ml of 0.3M h2so4 .What is the pH if the solution is…

A: Given  Millimoles of H2SO4 = M x V = 0.3 x 76  = 22.8 mmol Millimoles of H+ ion = 2 x millimoles of…

Q: How many moles of NH3 must be dissolved in water to give 819.8 mL of solution with a pH of 10.97? K,…

A:

Q: A 0.632 M solution of a monoprotic base has a pH of 11.53. What is the ionization constant of this…

A: Using pH we will get the consentration of OH-. Now since its a monoprotic base. means it will look…

Q: An aqueous solution contains 0.461 M ammonla. Calculate the pH of the solution after the addition of…

A: The concentration of ammonia = 0.461 M = 0.461 mol/L (M = mol/L) The number of moles of hydrobromic…

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: what is the pH of buffer solution containing 10.0g ammonium chloride to 250 mL of 1.0M ammonium…

A:

Q: A 0.285−mol sample of HX is dissolved in enough H2O to form 605.0 mL of solution. If the pH of the…

A: Dissociation extent for any species is clearly visible in its dissociation constant value. If this…

Q: When titrating 15 mL of hydrazoic acid (HN3) 0.000489 mol/L, with KOH 0.000517 mol/L: What is the…

A: Here we are required to find the pH of the solution

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: 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: Calculate the pH of a solution obtained by mixing 449 mL of0.17 M nitric acid with 405 mL of 3.6 x…

A: Since both the acid and base are strong in nature  Hence they will react until one of them gets…

Q: 0.00026 moles of acetic acid is added to 2.5L of water. What is the pH of the solution?

A: Acetic acid also called Ethanoic acid(CH3COOH )is a weak acid and on ionization it does not fully…

Q: A solution containing 572.0mL of 0.6309 M HCl is diluted to a volume of 1.000 L. What is the pH of…

A: "pH" is utilized to analyze the quantity of [H+] ion in concentration term in any solution. It…

Q: A solution is made by dissolving 27.5 g of HONH,CIO, in 500.0 ml. of water. Using Ka(HONH, ")-9.1…

A:

Q: What is the pH of a 50 cm3 KOH solution if the concentration of it is 0.0100 mol/dm3. How the pH is…

A:

Q: An aqueous solution at 25 ∘C is 14.7% HNO3 by mass and has a density of 1.043 g/mL. What is the pH…

A: The acidity of a solution depends on the concentration of the [H]+ ion. The pH is the most…

Q: A solution is prepared by mixing 25 mL of 0.06 M NaOH with 65 mL of 0.125 KOH. What is the pH of…

A:

Q: Given a mixture of 100cm3 of 1.01M HCl and 400cm3 of 0.04 NaOH, calculate the pH of the solution.

A: We have given that Volume of HCl = V1 = 100ml Molarity of HCl = M1 = 1.01M Volume of NaOH = V2…

Q: In the laboratory, a general chemistry student measured the pH of a 0.453 M aqueous solution of…

A:

Q: An aqueous solution at 25 °C is 14.4% HNO, by mass and has a density of 1.054 g/mL. What is the pH…

A:

Q: A solution is prepared by mixing 400 mL of 0.500 M NH3 and 195 mL of 0.500 M HCI. Assuming that the…

A: Given-> Volume of NH3 = 400 ml Molarity of NH3 = 0.500 M Volume of HCl = 195 ml Molarity of HCl =…

Q: A solution of cadmium hydroxide with a pH of 9.36 is to be prepared. What mass of cadmium hydroxide…

A: Given that: pH of cadmium hydroxide = 9.36  volume of solution = 1.50 L To find, the mass of…

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 is made by mixing 0.05 mL of 1.0 M HCI with 999.95 mL of pure water. Calculate the pH of…

A: The pH of a solution is the negative logarithm of hydrogen ion concentration.

Q: Calculate the pH of a solution obtained by mixing 438 mL of 0.14 M  nitric acid with 385 mL of…

A:

Q: A 0.15 M solution of a certain weak acid has a pH of 4.25. The K, of the weak acid is

A:

Q: If a buffer solution is 0.280 M in a weak acid (?a=1.6×10−5) and 0.510 M in its conjugate base, what…

A:

Q: A solution is prepared by mixing 0.2 moles of HCl into water until the final volume of the solution…

A: pH = -log[H3O+]  This formula is used to calculate to pH .

Q: Calculate the pH of the resulting solution when 35.00 mL of 1.000 M KOH is mixed with 65.00 mL of…

A: Given :  Molarity of KOH solution = 1.000 M Volume of KOH solution = 35.00 mL  Molarity of HCl…

Q: An aqueous solution at 25 C is 110% HNO, by mass and has a density of 1.046 g/mlL. What is the pH of…

A: Molarity of a solution is the number of moles of solute present in 1 liter of solution. The pH scale…

Q: How many moles of conjugate base should be added to 315 mL of 0.45 M HLac to give a pH of 4.00?

A: pKa of HLac = 3.85  Moles of HLac = 0.45 x 0.315 = 0.14175 mol Let moles of conjugate base ( Lac- )…

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: Enough of a monoprotic acid is dissolved in water to produce a 1.67 M solution. The pH of the…

A: 1- First calculate the H+ ion Concentration :  We know that, pH = -log([H+])  -pH = log([H+])  [H+]…

Q: A solution is prepared that is initially 0.069M in ethylamine (C,H,NH,), a weak base, and 0.15M in…

A:

Q: An aqueous solution contains 0.301 M hydrocyanic acid. Calculate the pH of the solution after the…

A: Given-> Molarity of HCN = 0.301 M Volume of HCN = 125 ml = 0.125 L (1L = 1000ml) Moles of KOH =…

Q: Enough water was mixed with 1.26 g of sodium hydroxide (40.0 g/mol) to make a 500. mL solution. What…

A:

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.