2.30 mL ofa 0.4375 M HCl 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: The pH of a solution that contains 0.010 M H3O+ is

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

Q: If the ?b of a weak base is 3.6×10−6, what is the pH of a 0.35 M solution of this base?

A: In order to figure out any certain basic solution's pH, first evaluate the hydroxide ions levels…

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

A:

Q: What is the pH of a barium hydroxide solution obtained by dissolving 0.27 grams of barium hydroxide…

A:

Q: how many mL of a .200 M HCl solution must be mixed with 12.0 mL of .1 M NaCN solution to give a…

A:

Q: The pH of a 0.0030 M solution of Ca(OH), is

A:

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

A: We know that  pH + pOH = 14

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: The pH of a basic solution is 10.33. What is [H]?

A: Given details, The pH of the base solution [OH-] = 10.33 To calculate the [H+].

Q: The pH of a basic solution is 9.93. What is [OH ]?

A:

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: If the ?b of a weak base is 6.2×10−6, what is the pH of a 0.10 M solution of this base?

A: From given  Kb of weak base is 6.2 ×10-6  By using base dissociation constant formula and from the…

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

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

A:

Q: An aqueous solution at 25 °C is 12.9% HNO, by mass and has a density of 1.049 g/mL. What is the pH…

A: Assuming we have 100 g of solution  hence mass of HNO3 in it = mass % X mass of solution / 100 =…

Q: To increase the pH of 1.50 L of 0.25 M HCIO3 (aq), which of the following would you add to the…

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Q: The pH of a basic solution is 12.77. What is [H*]?

A: The pH of a solution is mathematically expressed as: pH=-log[H+]   ............... (1) where [H+] is…

Q: A solution is prepared by dissolving 0.00050 mol KOH in enough water to prepare 500.0 mL of…

A: The pH is a scale that is widely used to measure the acidity or basicity of a solution. The pH is…

Q: If the ?b of a weak base is 6.7×10-6, what is the pH of a 0.26 M solution of this base?

A: Since it is not given whether the base is monoprotic or not. Hence we can assume it to be monoprotic…

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

A: pH + pOH = 14

Q: w When 10.0 mL of a 0.10 M HCI solution is diluted to 1.00 L, what is the pH of the new solution?

A: Given :- initial concentration of HCl solution = 0.10 M  Initial volume = 10.0 mL  Final volume =…

Q: The pH of a basic solution is 10.89. What is [H*]?

A: The pH of any solution is given by  pH = -log[H+] where [H+] = concentration of H+ ions in the…

Q: The pH of an aqueous solution of 0.549 M hydrocyar

A: HCN is a weak acid , weak acid does not dissociate completely hence it's pH can be calculated as…

Q: A solution is made by dissolving 0.0860 moles of Ba(OH)2 in enough water to make 755 mL of solution.…

A: Given information,    0.0860 moles of Ba(OH)2    Volume of solution is 755 mL

Q: The pH of a basic solution is 11.45. What is [H⁺]?

A: From  the definition of pH,the negative logarithm of concentration of [H+] is the pH of the…

Q: An aqueous solution of 0.40M Mg(C6H5COO)2 has a pH of__________.

A: Given: The concentration of Mg(C6H5COO)2 0.40 M To find: pH Formula:

Q: The pH of a basic solution is 12.83. What is [OH ]?

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration 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: An aqueous solution contains 0.411 M Na,HPO4 and 0.436 M H,PO4. The pH of this solution is

A:

Q: 50.00 mL of 0.0215 M HCI (aq) is mixed with 75.00 mL of 0.0200 M KOH(aq). What is the pH of the…

A: Given, For HCl solution, Molarity of the HCl solution = 0.0215 M = 0.0215 mol/L Volume of the HCl…

Q: If 215 ml of a .01M HBr is reacted with 250 ml of a .007M solution of KOH, what is the resulting pH?

A: HBr    +      KOH            →           KBr  +  H2OINITAL         215×.01…

Q: If the ?b of a weak base is 1.7×10−6, what is the pH of a 0.18 M solution of this base?

A: The base dissociation constant is Kb, which indicates the dissociation of base in water. The…

Q: The pH of a basic solution is 12.59. What is [OH⁻]?

A: Given: The pH of a basic solution is 12.59 [OH-] is the concentration of hydroxide ion

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

A: Introduction If the value of hydronium ion of any particular solution is known then one can easily…

Q: What is the pH of a solution in which 43 mL of 0.33 M NaOH is added to 13 mL of 0.170 M HCl?

A: Moles of NaOH and HCl are determined as follows,

Q: A solution containing 175mL of 1.50MHBr is diluted to a volume of 1.00L. What is the pH of this…

A: Given, M1 = 1.50 M V1 = 175 mL V2 = 1.00 L M2 = ?

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

A:

Q: What mass in grams of nitric acid is present in 700 mL of a solution with a pH of 1.866?

A:

Q: The concnetration of NaOH solution is 1.0 M. What will be the pH of solution?

A: NaOH is a strong base , so we would first calculate its pOH using the formula : pOH = - log [OH-]…

Q: The pH of a basic solution is 12.39. What is [H*]?

A: The question is based on pH determination of a solution pH is defined as negative logarithmic of…

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: 1.00 L of hydrochloric acid is prepared and has a final pH of 1.045. What mass of HCl) is dissolved?…

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: 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…

Q: A solution contais 0.0111 grams of strong base calcium hydroxide completely dissolved in 635 ml of…

A: Given,Calcium hydroxide = 0.0111 grams,Volume = 635 ml.Molar mass of 74.093 g/mol.Equivalent Weight…

Q: The pH of a basic solution is 11.43. What is [OH⁻]?

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.