Phosphoric acid (H3PO4) is a triprotic acid with the following K₂ values: Ka1 = 7.5x10-3 Ka2 = 6.2X10-8 Ka3 4.8x10-13 = What is the concentration of the phosphate ion (PO43) in a 0.86 M NaH2PO4 solution? 7.5x10-3 6.2X10-8 4.8x10-13 none of the above

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.26 M solution…

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Q: calculate the equilibrium constant for the reaction

A: We are given  concentrations of H+ and Al(H2O)5OH2+ are found to be (2.74x10^-3) M  (1.3x10^-1) M in…

Q: Over-the-counter (OTC) antacids are chemicals that neutralize acidity to relieve a painful reflux.…

A: Antacids :Our stomach produces hydrochloric acid(HCl). It  helps in the digestion of food without…

Q: The pH of an aqueous 0.0100 M solution of NaOH is: 2 O 12 01 OO 07 9

A: The objective of the question is to determine the pH of a 0.0100 M NaOH solution and to identify…

Q: For the diprotic weak acid H2A, ?a1=3.7×10−6 and ?a2=6.2×10−9. What is the pH of a 0.0450 M…

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Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.60 M solution…

A: Answer:Value of pH is equal to:

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.23 M solution…

A: The PH of diprotic acid can be calculated as follows

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.18 M solution…

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Q: Find the [H3O+][H3O+] concentration of a 0.290 M M  acetic acid solution. (The value of KaKa for…

A: Given, the concentration of acetic acid =0.290 Mand Ka for  acetic acid =1.8×10-5 we are asked to…

Q: What is the hydronium ion concentration of a solution with [OH–] = 1.75 x 10-9.

A: Concept: Water undergoes auto-ionization as shown in the following equation. 2 H2O  -->   H3O+ +…

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.14 M solution…

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Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.45 M solution…

A: The question is based on the concept of equilibrium. we have determine the pH of the given diprotic…

Q: Arsenic acid, H3AsO4, is used industrially to manufacture insecticides. Arsenic acid is a polyprotic…

A: The concentration of the HAsO42- is to be calculated in a solution whose initial arsenic acid…

Q: An acetic acid solution has a pH of 5.80, what is the [OH-] in this solution?   A 1.6  x 10–20 M…

A: pH is a scale to measure the concentration of hydrogen ions. The negative logarithm of hydrogen ion…

Q: The concentration of hydroxide ion in an aqueous solution at 25°C is 3.9 × 10⁻⁴ M. What is the…

A: Given :  Temperature = 25 °C  [OH-] = 3.9 x 10-4 M

Q: How many moles are there in 20.0 mL of a 0.125 M solution?

A: Molarity = moles of Solute ÷ Volume of solution(L)

Q: At the same concentration, which of the following aqueous solutions has the lowest pH? O HNO3…

A: pH stands for power of hydrogen. pH is defined as negative of logarithm of hydrogen ions.…

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.20 M solution…

A: Reactions- H₂A + H2O ↔HA-  + H3O+  Ka1 = 3.4 × 10⁻⁴ HA- + H2O ↔ A2- + H3O+  Ka2 = 6.7 × 10⁻⁹ Ka1…

Q: Calculate the percent ionization of a 1.00 M solution of hydrocyanic acid, HCN.

A: According to Bartlby guidelines i solve only first question.You post  Second question  separately.

Q: What is the concentration of X2- in a 0.130 M solut Ka2 = 7.5 x 10-11. O 1.6 x 10-8 M 6.2 x 10-4 M O…

A: H2A H+ HA- I 0.130 0 0 C -x +x +x E 0.130-x x+y x+y Further dissociat is   HA- H+ A2,-…

Q: CALCULATE THE [H30+] CONCENTRATION OF A SOLUTION WITH A PH OF 5.5

A: Given pH = 5.5

Q: What is the hydronium ion concentration in 0.275 M nitrous acid? Ka= 7.1x10^-4

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Q: Assuming complete dissociation, what is the pH of a 3.67 mg/L Ba(OH)₂ solution? pH =

A: The mass of barium hydroxide = 3.67 mg =         ( 1.0 mg = 10-3 g)Molar mass of Ba (OH)2, = 171.34…

Q: The OH⁻ concentration in an aqueous solution at 25 °C is 3.5 × 10⁻⁵. What is [H⁺]?

A: We have to calculate the hydrogen ion  Concentration.

Q: The concentration of hydroxide ion in an aqueous solution at 25°C is 3.5 × 10⁻⁴ M. What is the…

A: Given, Concentration of hydroxide ion = [OH-] = 3.5 × 10-4 M Concentration of hydronium ion = [H3O+]…

Q: What is the pH of an aqueous solution of 2.37×10-2 M nitric acid? pH =

A: The important thing to keep in mind here is that nitric acid is a strong acid, which means that it…

Q: What salt is formed in the following acid-base reaction? LiOH (aq) + H3PO4 (a 4 (aq) Give the…

A: Acid base reaction is the chemical reaction in which an acid reacts with a base to form a salt and…

Q: Each of the four flasks below contains the same volume of .10 M aqueous acid. All four acids are…

A: Since the volume and concentration of acid taken is same for all acids  Hence the moles of all acid…

Q: A solution has a hydronium concentration of 7.50 x 10-5. What is the hydroxide concentration in M?

A: Given = Hydronium ion concentration (H30 +) =7.50*10-5 Hydroxide ion concentration (OH-) =?

Q: A diprotic acid (H2AH2A) has ?a1=4.73×10−7Ka1=4.73×10−7 and ?a2=6.09×10−11.Ka2=6.09×10−11. What is…

A: pH is defined as the negative logarithm of hydrogen ion concentration. It can be given as  pH=-log…

Q: Assuming complete dissociation, what is the pH of a 4.04 mg/L Ba(OH)2 solution? pH=

A: Given :  We have to calculate pH.

Q: The concentration of hydroxide ion in an aqueous solution at 25°C is 3.6 × 10⁻⁴ M. What is the…

A: The concentration of the species gives the amount of that species used in the desired reaction.…

Q: Which solution below has the highest concentration of hydroxide ions? pH = 8.2 pH = 5.6 pH = 3.7 pH…

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Q: The concentration of hydroxide ion in an aqueous solution at 25°C is 5.2 × 10⁻⁴ M. What is the…

A:

Q: -8 An aqueous solution at 25 °C has a OH concentration of 1.7x 10 °M. Calculate the H,0' concentrati…

A: [OH-] = 1.7 × 10-8 M Temperature = 25 °C [H3O+] =?

Q: The H* concentration in an aqueous solution at 25 °C is 2.5 × 104 M. What is [OH]?

A:

Q: Assuming 0.1 M concentrations, arrange the following acid solutions in order of increasing pH.…

A: Concentration of each given acid = 0.1 M (c) We know that -> [H+] = √(Ka ×c)

Q: 8. The compound Mg(OH)2 is classified as an Arrhenius base because, when dissolved in water, there…

A: According to the Arrhenius theory, the substance that gives hydrogen ion H+ in the aqueous solution…

Q: Which of the following characteristics of perchlorate (CIO4) best explains why perchloric acid…

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Q: Given 0.01 M solutions of each of the following acids, which solution would have the lowest pH? O…

A: The objective of the question is to determine the solution with the lowest pH.

Q: Assuming complete dissociation, what is the pH of a 4.12 mg/L Ba(OH)₂ solution? pH =

A:

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.46 M solution…

A: For first ionization, [H+] = (Ka1 * C)^1/2 where C = initial concentration of acid = 0.46 M [H+] =…

Q: What is the hydronium ion concentration of a 0.010 M solution of acetic acid? Ka for acetic acid is…

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Q: Assuming complete dissociation, what is the pH of a 3.73 mg/L Ba(OH)₂ solution? pH: =

A:

Q: The H⁺ concentration in an aqueous solution at 25 °C is 5.5 × 10⁻⁴. What is [OH⁻]?   What is the…

A: 1) [H+] =5.5×10-4 M [OH-] = ?

Q: 6.7

A: Here : O.35 M = C ( original concentration )  [H+] = √( Ka1 • C )  Using this formula, Calculate…

Q: Phenol (C6H5OH), commonly called carbolic acid, is a weak organic acid. C6H5OH(aq) + H₂O(l) C6H5O¯…

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.