Solve using step-by-step process (solutions). 1. What is the pH value and what is the hydroxyl-ion concentration of a solution that is 0.0010 M in HCl? (Ans. pH = 3.0 ; [OH-] = 1.0x10 -11 )   2. The pH value of a certain solution is 5.92. What are the pOH value, the hydrogen-ion concentration and the hydroxyl-ion concentration? (Ans. pOH = 8.08 ; [H+] = 1.20x10-6 M ; [OH-] = 8.3x10-9 M)

Q: What is the pH of a 0.16 M NH3 solution? Kb = 1.8 x 10-5 (at %3D the current temperature) IMPORTANT:…

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Q: 73. Calculate the pH of each solution. (a) [OH-] = 1.9 × 10-7 M (b) [OH-] = 2.6 × 10-8 M (c) [OH-] =…

A: To find out pH of a given solution, first calculate pOH of the given solution. Using the relation…

Q: 15) Which of the following is the weakest acid? SH OH NH, d) SH

A: From given compounds there is need to find weakest acid among all compounds.

Q: ..A 1.68 M solution of a weak acid HA is found to have a pH of 2.09. Determine K, of the acid…

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Q: Does the pH of a solution increase or decrease when a strong acid like Hydrochloric acid (HCl) is…

A: We know the relation between the concentration of hydrogen ion and pH of solution→…

Q: 2. Complete the following table with the appropriate values with appropriate units and sig figs (if…

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Q: 1.What is the pH of a 0.240 M aqueous solution of sodium cyanide, NaCN? pH =  This solution is .

A: 1. Given that Concentration of NaCN solution [C]= 0.240 M pKa of HCN = 9.22    NaCN     ​+    ​H2​O​…

Q: Q6. i. Convert the below-given pOH values to corresponding (H*] and [OH'] values: a) 10.8 b) 3.8 ii.…

A: The given problem can be solved by using the formula given below as;

Q: Calculate the PH and pOH for eacho the solutions with the fo11owing hydngo 1on or hydrxide ion…

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Q: 51. Fill in the missing information in the following table. Acidic, Basic, or pH pOH [H+] [OH]…

A: The pH of a solution can be calculated as follows: pH=-logH+ We know that; pH+pOH=14 The pOH of the…

Q: Which one of the following aqueous solutions has the highest [OH-]?? A .a 1x10-3 M solution of…

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Q: What is the pH of 0.5956 M solution of NaCl at 25 0C? pH = ?

A: The pH of any solution is defined as the negative log of Hydrogen ion concentration.

Q: 3) A solution has a pOH of 3.62. b. Calculate the pH of the solution. c. Explain whether the [H*] or…

A: Given:- pOH = 3.62 pH + pOH = 14

Q: Four so v s of an acid dissolved in water are sketched below, as if under a micoscope so powerful…

A: There are two types of bases/acids. One is strong base/acid which is completely dissociable in into…

Q: Solution A has a pH of 5.6. Solution B has a pH of 2.8. Which has a higher (H*] concentration? O…

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Q: The [OH-] = 5.4 x 10-5 M for the NH3 and NH4Cl solution. What is the pH of the solution? pH = [?]

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Q: The pH of a basic solution is 11.59. What is [H*]? 5. The pH of an acidic solution is 4.59. What…

A: pH = -log[H+] [H+

Q: For a solution that is 0.164 M NH3 and 0.102 M NH4Cl, calculate the [OH-].  NOTE: You may enter a…

A: Given,  [NH3] = 0.164 M  [NH4Cl] = 0.102 M  Calculate the [OH-] = ?  Use Henderson-Hasselbalch…

Q: 17. If the pOH of a solution is 4.52, calculate the pH, the [H'] and the [OH].

A: Determine the pH of the given solution from pOH using the below formula.

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

A: Given:- For a solution in a container,  No of moles of HCl = 2.60 x 10-3 No of moles of NaOH = 3.32…

Q: 35. What is the pH of the resulting solution when 0.20 mol of HCl is added to 0.250 L of water?

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Q: A solution is found to have a pH of 8.3, what is the hrdroxide ion [OH-] concentration?

A: Introduction If we know the pH of any particular solution, then first [H+] is calculated then with…

Q: To add an O atom in basic solution, add 2 OH to the side that needs the O atom, and also add an H,0…

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

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Q: pOH

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Q: Calculate the pH and pOH of the following solutions. Report your answers to 3 sig figs. a) 0.00640 M…

A: pH : pH can be defined as the negative logarithm of hydrogen ion (H+) concentration.pH = -log[H+]…

Q: 36. Which will have a lower (the lowest) pH among the solutions shown in each of the following…

A: a) 0.001 M NaOH and 0.005 M NaOH  Since NaOH is a strong base hence it will dissociate completely…

Q: Calculate the pOH of a solution that is 9.45x10-12 M of Potassium hydroxide (KOH). pOH=    (round…

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Q: Determine the (H*|. (OH], and pOH of a solution with a pH of 12.26 at 25 °C. [H*| = %3D (OH-| = POH…

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Q: Calculate the pH of the solution after the following addition to the 42.0 mL of 0.135 M HCI: C) 37.8…

A: Given data,molarity of HCl = 0.135MVolume of HCl=42.0mL = 0.042LMolarity of NaOH=0.150MVolume of…

Q: -117. Determine [OH¯], [H*], and the pH of each of the following solutions. a. 1.0 MKCI b. 1.0 M…

A: Given,1.0 M KCl1.0 M KC2O2

Q: 2. What is the pOH of a 0.0235 M HCl solution? 3. What is the pH of a 6.50 x 10-3 M KOH solution?…

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Q: 14. The pH of grapefruit juice is 4, what is the pOH?-18X3 1x1044 1x104 15. What is the…

A: Given,  The pH of the grapefruit juice is 4, The pOH of the solution is:

Q: KNO, HNO, MgF2 NaOH

A: From given  Each compound is given a name and  checked whether it is ionic, molecular, acid, base…

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.