The K, for hypoiodite anion (IO) is 4.35x10-4. What is the pH of a 0.226 mol L solution of lithium iodate solution? O 4.008 2.004 O 11.996 O 9.992 O 12.319

Q: Calculate the [H3O+], [OH-], pH and pOH of  a 0.120 M HNO2  (nitrous acid).  Ka = 7.10 x 10-4

A: The given data contains, Ka= 7.10×10-4 Concentration of HNO2 = 0.120 M

Q: What is the pH of 6.0 x 104 M HF? The K, for hydrofluoric acid is 7.2 x 104. O a. 2.95 b. 3.22 C.…

A: Answer:- This question is answered by using the simple concept of ionisation of weak acid and then…

Q: Calculate the pOH of the following aqueous solutions at 25°C: (a) 0.013 M LiOH, (b) 0.013 M Ba(OH)2…

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Q: The K, for dihydrogen borate anion (H,Bro,) is 1.72x105. What is the pH of a 0.188 mol L solution of…

A: For salt of weak acid & strong basepH = 12pKw + 12pK + 12logcc = concentrationKa = acid…

Q: White vinegar has a pH of 2.4 while apple cider has a pH of about 4.25. What is the difference…

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Q: 10. A 0.045 M solution of hypobromous acid (HBrO) has a pH of 5.02. Calculate the K, for hypobromous…

A: According to the question, the balanced chemical reaction is: HBrO(aq) + H2O(l)   ---->  H3O+(aq)…

Q: The pH of a 0.064-M solution of hypobromous acid (HOBR but usually written HBrO) is 4.97. Calculate…

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Q: What is the [H+] for a solution with a pH of 5.2? * O 0.7 O 6.3 x 10A-6 8.8 O 1.6 x 10^5 What is the…

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Q: What is the pH of a 0.50 M solution of Ca(OH)2? 14.00 O 0.30 1.00 9.70

A: Ca(OH)2 is a strong base , but less soluble base. But since it is strong base, all the Ca(OH)2 which…

Q: The pH of a 0.063-M solution of hypobromous acid (HOBR but usually written HBRO) is 4.93. Calculate…

A: We will use weak acid concept.

Q: Find the pH of 0.180 M NACN solution. For HCN, K = 4.9 x 10 10 O 8.57 O 2.72 O 5.03 O 11.28

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Q: What is the pH of a 0.015 M HCIO4 solution? a. 1.82 O b. 12.18 C. 0.015 d. 0.030

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Q: An aqueous solution has hydronium concentration [H3O+] = 9.8 x 10-5 mol L-1. What is the pH of the…

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Q: What is the pH of a 0.0040 M Sr(OH)2 solution? O 12.00 O 2.40 O 11.60 O 11.90 O 2.10

A: Strong acids or bases  are dissociated completely. so we can direct calculate its [H+] or  [OH-]…

Q: What is the pH of an aqueous solution that is 0.123 M NH4Cl? (Kb for NH3= 1.8 x 10^-5)

A: Solution :         The pH of an acid or base can be calculated by using hydronium ion…

Q: Which solution below has the lowest concentration of hydroxide ions? O pH=7.93 O pH=10.12 O pH=7.00…

A: PH is defined as the negative logarithm of Hydrogen ion concentration.  PH = - log ( H+ )…

Q: PH of a solution whose OH ion concentration is 0.010 m/l 10-12 O 10-3 O 12

A: pH of the solution = 12    Answer is 'more reactants'

Q: 7) What is the pOH of a solution with a pH of 3.7? A) 14.0 B) 2.5 C) 10.3 D) 0.115 E) 0.25

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Q: A sample of fruit juice is found to have à hydrogen concentration of 2.87 x 104. What would the pH…

A: Given hydrogen ion concentration of fruit juice is 2.87*10-4. We have to determine PH of fruit…

Q: A solution is made by dissolving 18.4 g HCI (MM=36 g/mol) in 662 mL of water. The pH of the solution…

A: HCl is strong acid

Q: HCl is a strong acid.  What is the pH of a solution of concentration 1 x 10-3M?

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Q: 13. What is pH of a 0.25 M sodium hydroxide solution?

A: Since you have asked multiple questions, we will answer the first question for you. For any specific…

Q: 13. A solution of hypochlorous acid HClO(aq), has a concentration of 0.100 mol/L. If the pH of the…

A: Given: The concentration of HOCl = 0.100 mol/L The pH of the solution = 4.23 We have to calculate…

Q: A solution has [OH¯] = 5.2 × 10-4 M. The pH of this solution is O 1.92 × 10-11 O 10.72 O None of…

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Q: The concentration of H* (or H3O*) from part A should be 1.02x×10-2 mol L-1. What is the pH of the…

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Q: Which of the following indicates the most acidic solution? A. [OH]=0.5 M B. [H] =0.3 M C. pOH = 5.9…

A: pH = - log [H+] pOH = - log [OH-]   [OH-] = 10-pOH  [H+] = 10-pH    pH + pOH = 14    pH = 7 :…

Q: Hydrogen lon Concentration pH Basic/Acidic 1.0.0015 2. 5.0x109 3. 1.0 4. 1.0x10-12 5. 0.0001 6. 1.00…

A: The pH of a solution is calculated by taking negative log of the concentration of hydrogen ions.  If…

Q: Calculate the pH and the pOH of each of the following solutions at 25°C for which the substances…

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Q: Calculate the pH and pOH for the solution with [Ca(OH)2]= 4.29x10^-5M Is the solution acidic or…

A: The value of pH can be determined by the concentration of the hydrogen ion present in the solution…

Q: What is the pH of a 0.780 M solution at 25 oC?   (  Ka = 4.9 x 10−10, at 25 oC)

A: Given, concentration of a solution (c) = 0.780M dissociation constant of acid (Ka) = 4.9×10-10

Q: UESTION 7 Determine the hydronium ion concentration for solutions with the following pH values: a.…

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Q: Use the data in Table 15.2 to determine the equilibrium constant for the reaction. HCIO2 (aq) + NO…

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Q: Calculate the percent ionization of a 0.125-M solution of nitrous acid (a weak acid), with a pH of…

A: pH of a solution is equal to negative logarithm of the concentration of the hydrogen ion. Write the…

Q: 1.0 x 10 11 moles of HCl are added to 1.0 L of H2O. What is the pH? O 10.0 O 11.0 3.0 o 7.0

A: Moles of HCl = 1.0 × 10^-11 mole Volume of H2O = 1.0 L

Q: Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid…

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: What is the pOH of a 0.16 M solution of hydrazoic acid? A) 2.76 B) 5.52 C) 8.48 D) 10.74 E) 11.24

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Q: A 0.00653 M solution of an unknown weak acid has a pH of 3.510 at 25 °C, what is the K acid at 25…

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Q: Explain what happens to the ratio of the two common forms of free residua! chlorine as the pH of…

A: Hypochlorite, ClO-(aq) is a conjugate base of HOCl.  #(i): Since HOCl(aq) and ClO-(aq) are conjugate…

Q: The pH of a 0.01 M HNO2(aq), Ka=4.0x10^-4  ,solution is in which of the following ranges?  a.)…

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Q: Calculate the pH and pOH for each of the solutions with the following hydrogen ion or hydroxide ion…

A: The equations which we relate pH and pOH are  pH + pOH = 14 And the pH and pOH of any solution is…

Q: 25) Which of the following ions will act as a weak base in water? A) CIO- B) Cl- C) NO3- D) OH- E)…

A: Powerful acids are an acid that dissociates in water almost entirely or almost completely. An acid…

Q: H2Se is a diprotic acid. What is the pH of a 0.10 M H2Se solution ? Kal = 1.3 x 10-4 and Ka2 = 1.0 x…

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Q: The pOH of an acidic solution is 10.15. What is [OH⁻]?

A: pOH of any solution is given by  pOH = -log[OH- ] where [OH- ] = concentration of OH- ions in the…

Q: 16. For Nis) + 2H* (? M) H2 (1 atm) Ni*2 (1 M) E = .01v Calculate the pH of the solution.

A: Given reaction: Ni(s) + 2H+(aq) → H2(1 atm) + Ni2+(1 M) E = 0.01 V We have to calculate the pH of…

Q: A solution has a pH of 3.66. The pOH of this solution is O 10.34 O 10.24 none of these O 3.76 O 3.66

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Q: At 25 °C, which aqueous solution has the lowest pH? O 0.17 M HNO2 O 0.15 M HNO3 O 0.20 M HCOOH O…

A: We know that pH of acid is less than 7 and pH of base is greater than 7. As the strength of acidity…

Q: Determine the pOH of a 0.461 M C,H5 COOH solution if the Ka of the acid is 6.5 X 10-5 5.48 O 11.74…

A: We will first write dissociation equation of acid, then calculate H+ concentration to find pH and…

Q: What is the pH of an aqueous solution at 25.0 °C in which [OH ]is 0.0045 M? O 2.35 O -11.65 O 11.65…

A: Answer: option c) 11.65 is the pH of the solution.

Q: A 0.05 molar acidic solution has an ionization constant of 2.50 x 10-5 , what is the concentration…

A: Leta consider Acid is a monoprotic Acid Ionisation constant = 2.50 × 10-5Concentration of Acid =…

Q: A 0.10 M solution of an acid has a pH of 3.0. The percent lonization is O 1.0 O 3.0 O 0.010 O 0.30

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.