The pH of a solution is 2.55. What is the[H3O+] A 2.8x10-3M B 2.55M C 2.0x10-15M D 0.28M

Q: pH of solution with an H3O+ concentration  [H_3O^+]= 1.00 x 10^-2 M [H_3O^+]= 5.42 x 10^-12 M

A: pH is termed as the negative logarithm of hydrogen ion concentration. It can be calculated as: pH =…

Q: A sample of a cleaning product containing household ammonia, has a pH of 10.5. Determine the…

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Q: What is the pH of a solution containing the following: a. 80 mM H* b. 2x10-2 mg/LH c. 6x10- mg/L OH

A: The solutions given are,

Q: A solution has a [H3O+] of 1 × 10−3 M. What is the [OH−] of the solution?  A)11 M  B)14 M  C)1 ×…

A: Given : [H3O+] = 1 × 10−3 M.            =10−3 M.

Q: A solution has a pH of 7.68. A) the solution is very acidic B) the solution is only sightly acidic…

A: We have to identify the following given options have a solution has a pH of 7.68 as follows in step…

Q: What is the [OH] in a solution with a pH of 9.22? (1.7 X 10 M)

A: Given that pH of solution=9.22

Q: Determine the pH of a 0.048 M hypobromous acid (HBrO) solution. Hypobromous acid is a weak acid (Ka…

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Q: 5. Determine the pH of each solution: a. [H*] = .0026 M b. [OH] = 3.2 x10-M

A: The pH of the solution is determined as- pH = -log [H+]

Q: 10. If the pH of a solution is 6.6, determine the hydroxide ion concentration. A. 1.00 x 10-7 M B.…

A: We need to find hydroxide ion concentration in solution.

Q: Calculate the molar H3O* ion concentration of solution that has a pH of (a) 9.21 (b) 0.45 (c) 7.32…

A: pH: It can be defined by saying the power of hydrogen in any compound. It ranges from 0 to 14. We…

Q: What is the pH of a 0.0758 M solution of NH4Cl? Kb for NH3 = 1.8 × 10−5

A: NH4Cl is salt of strong acid and weak base

Q: What is the H3O + concentration of an aqueous solution with a pH of 12.17 A. 6.8x10-13 B1.9x10-9…

A: Answer :  We have to calculate Concentration of H3O+ and pH of solution is given I.e 12.17

Q: Calculate the pH of a 0.307 M NH3 solution. NH3 has a ?b=1.8×10−5.

A: First of all a balanced reaction should be written for the solution: Here, water concentration is…

Q: Calculate the theoretical pH of each solution. 0.100 M aluminum nitrate Hydrated aluminum ion –…

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Q: Which best describes the pH value of a solution with a H3O+concentration of 1.68 * 10 -5M? a. pH =…

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Q: What is the PH of each of the followig?   (a)  0.0010 M HCl (b)  0.76 M KOH (c)  2.8x10^-4 M…

A: The pH of a given solution can be termed as a measure of its basicity or acidity. It is a measure of…

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: What is the pH of a solution that is 3.0 M H2SO4

A: Please find the solution below:

Q: Determine the concentration of H+ in each solution at 25°C. A solution with pH = 1.0. [H*] : M A…

A: Given,  pH  of solution = 1.0 [H^+] =?

Q: What is the pH for a 0.05M solution of hydrochloric acid (HCI)? O -0.3 O 6.95 0.05 1.3

A: HCl is a strong monobasic protonic acid.

Q: A sodium hydroxide solution has a pH of 12.40, what is the OH– concentration in this solution?

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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: 5.07 g of HCl(g) is dissolved in water to make a 220 mL solution. Calculate the pH of the solution.

A: Since you have posted multiple questions we are answering first question for remaining question to…

Q: 7. A base has % ionization of 0.3%. What is the pH of 0.05 M solution of the base? A. 1.3 В. 3.8 С.…

A: A base is a substance which produce OH- when dissolved in water. Let the given base be B which…

Q: what is the ph of a solution with (H3O+) = 2.8 *10^-9 M? a. -8.6 b. -5.4 c. 3.6 *10 ^-6 d. 5.4…

A: pH = -log(H3O+)

Q: 8. The normal pH of human blood ranges from 7.35 to 7.45. Calculate the concentrations of H3O* and…

A: Given,  pH  = 7.45 [H3O+] = 10-pH = 10-7.45 = 3.55×10-8 M   [OH-] = 10-14/[H3O+]  = 2.82 × 10-7 M

Q: Which of the following is amphoteric? OHCO3- О HCI NH4 O CO3²-

A: An amphoteric substance can function as either an acid or a base, depending on the media. Amphoteric…

Q: Calculate the pH of each of the following solutions: (a) 0.0010 M HCl (b) 0.76 M KOH

A: The pH and pOH of the solution can be determine by using the formula is as follows;

Q: Calculate the pH of the following solutions, a) 0.25 M H2SO4; b) 0.2 M KOH; c) 0.02 M HNO3; d) 0.1 M…

A: pH is  negative log of concentration of H+ ion. pH= -log[H+]  And also [H+][OH-] = 10-14 Where [H+]=…

Q: A solution has an OH- concentration of 1.0 x 10-3 mole/L. What is the solution's pH? a. 3.0 b. 4.0…

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Q: What is the pH of a solution that has an {H30*] = 5.9 × 10-/

A: Introduction: The pH is the concentration of hydrogen ion in gram equivalents per liter.it is a…

Q: Calculate the pH of a 0.645 M NH3 solution.NH3 has a ?b=1.8×10−5

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Q: If you have a solution with a [H+] of 6.87x10- M, what is the pH of the same solution? 9.16 6.16 O…

A: pH = - log [H+] pH = - log (6.87 x 10-5) pH = -[ log (6.87) + log (10-5)] pH = -[0.837 + (-5)] pH =…

Q: 27. Calculate the pH of each of the following solutions containing a strong acid in water. a) 2.0 x…

A: Strong acid dissociate and produce H+

Q: 6.7

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

Q: Which of the following chemical species is amphoteric? a. NaOH b. C4H10 c. H2O d. H2SO4   What is…

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Q: 9. What is the PH of a solution with [OH¯]=1 x 10ªM |10 |9HF O11HCNO |None of the others

A: Given, a solution having [OH-] =1×10-4 Mwe are asked to calculate the pH of the solution.

Q: What is the pOH of a solution that has ​[OH^-] = 2.7E-4 M

A: pOH can be expressed as -log[OH-]. It is used to represent basicity of a solution. If the pOH value…

Q: The pH of a solution is 4.80. What is the concentration of hydroxide ions in this solution? 4.2 x…

A: Given that, pH =4.80 Then, [OH-] = ?

Q: Which solution has the highest pH? A) 0.222 M HF B) 0.222 M HI C) 0.222 M HBr D) 0.222 M HClO4…

A: Acids are those compounds or molecules which liberate H+ ions in the aqueous solutions. Strong Acids…

Q: What is the pH of a 0.375 M solution of HF? Ka of HF = 3.5 × 10−4

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Q: What is the pH of a 3.1 x 10-3 M LiOH solution? a. 11.5  b. 2.51 c. 11.2 d. 2.64

A: To calculate the pH of an aqueous solution you need to know the concentration of the hydronium ion…

Q: The pH of a solution is 9.67. Calculate the hydrogen ion concentration in the solution. [H*] = 2.1 x…

A: The question is based on the concept of pH. It is defined as the negative logarithm of hydrogen ion…

Q: 3) Based on the value for [H3O*], calculate the pH of this 0.160 M HPro solution. 4) Calculate the…

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Q: Calculate the pH of solutions having the following [H+]: (a) 0.68 M (b) 1.42 M (c) 4.5 × 10-5 M

A: The pH is the negative logarithm of hydronium ion concentration. pH=-logH+

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: What is the pH of a solution of 0.010 M CH3NH3ClO3?    A. 8.54  B. 6.32 C.4.74 D.10.12

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Q: pH of a solution is 3.53. What is the OH⁻ concentration

A: [H+] = 10-pH [H+] x [OH-] = 1 x 10-14

Q: What is the pH of 4.50M H3PO4

A: Given,  Molarity of H3PO4 = 4.50 M pH = - log [H+]

Q: Human tears have a concentration of H3O+ that is 3.16 x 10-8. The concentration of OH-in human tears…

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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.