Calculate the pH of a solution that contains 11% (w/w) NaOH and a density of 1.05 g/ml?, MW 40 O a. 14.46 O b. 10.6 C. 0.56 O d. 13.8

Q: 11. The pH of a Ba(OH)2 solution is 10.00. What is the Ht ion concentration of this solution? A. 4.0…

A: pH is used to determine the concentration of hydronium ion.

Q: The pKa for HCN(aq) is 9.21. What is the pH of a 1.245 M solution of NaCN? O a. 11.25 O b. 1.24 O c.…

A: this is the salt of weak acid and strong base. so ,we will use hydrolysis equation of weak acid and…

Q: The K a of hydrofluoric acid (HF) at 25.0 °C is 6.8 × 10 -4. What is the pH of a 0.20 M aqueous…

A: Given, the Ka for hydrofluoric acid =6.8×10-4concentration of HF =0.20 Mwe are asked to calculate…

Q: Which aqueous solution has the lowest pH? O a. 0.30 M HCI O b.0.30 M NH 3 Oc.0.30 M CH 3COOH O…

A:

Q: 28. How many grams of NaOH must be added to 0.30 L of water to make a 2.0% (w/v) solution? A) 60. g…

A: 28. Given :- volume of water = 0.30 L  % w/v = 2.0 %  To calculate :-  Mass of NaOH

Q: e the pH of the solution. Be s

A:

Q: Calculate the mass of sodium hydroxide that the chemist must weigh out in the second step. Round…

A: NaOH sodium hydroxide is a strong base and dissociates completely in water .

Q: A 0.1 M solution of has a pH = 7.0 A. KF B. NaF C. NANO3 D. Na2S E. NH4CI

A: The given pH of the salt solution is 7.0, which is neutral. Thus, the salt which upon hydrolysis…

Q: 5. If 30 ml of a 0.58M solution of HF is reacted with 25 ml of a .65M solution of NaOH, what is the…

A: HF                    +             NaOH…

Q: III. A solution is made by adding 10-3 M HOCI and 10-3 M NaPr to water. Then, NaOH is added until…

A:

Q: Hq bn6 200116302210 6. A solution is prepared by mixing 90.0 mL of 5.00 M HCl and 30.0 mL of 8.00 M…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: A week diprotic acid H2A has Ka1 = 4.2 × 10–7 and Ka2 = 4.8 × 10–11. Determine the pH of a 0.17 M…

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Q: Calculate the H3O+ and pH of each polyprotic acid solution. a. 0.350 M H3PO4 b. 0.350 M H2C2O4

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Q: A solution containing 2.60 x 103 moles of HCl and 3.32 x 10~³ moles of NaOH into a container and…

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Q: 5. Acetic acid is a weak monoprotic acid. Its concentration is 0.20 M and its Ka value is 1.8x10-5…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: 1. Calculate the pH of the following: a. A solution whose pOH = 8.95 b. 6.37 M HCI c. 5.25 M Ca(OH)2…

A: pH : it can define as the negative logarithm of H+ ion concentration. When pH > 7 solution is…

Q: A week diprotic acid H2A has Ka1 = 4.2 × 10–7 and Ka2 = 4.8 × 10–11. Determine the pH of a 0.17 M…

A: Ka1 = 4.2 × 10–7     pKa1 = 6.376 and Ka2 = 4.8 × 10–11    pKa2 = 10.319

Q: Calculate the pH of a 1 x 10-5 M HNO, solution. a. 9 10 b.14 C. 5

A:

Q: Which of the following is the pH value of an aqueous solution with an OH- concentration of 0.00250…

A: pH or power of hydrogen is defined as the negative logarithm of hydrogen ion concentration present…

Q: The k A.

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.