If the ?b of a weak base is 5.0×10−6, what is the pH of a 0.28 M solution of this base?   pH=

Q: Calculate the pH of solutions having the following [H+]:   a) 1.69 M

A: Given : [H+] = 1.69M

Q: The pH of an acidic solution is 5.81. What is [H⁺]?

A: Given : pH = 5.81   We have to calculate Hydrogen ion concentration([H+]).

Q: Calculate the [H3O+] for a solution in which [OH -] = 2.7 x 10-11 M. Is this solution acidic, basic,…

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Q: For each conjugate acid-base pair, identify the first species as an acid or base and the second…

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Q: Which of the following statements describes a 0.010 molar weak acid solution? a) not enough…

A: pH of a solution is defined as the negetive logarithm of concentration of H+ ion.  Here the…

Q: Identify the acid and base on the left and the conjugate acid and conjugate base on the right:

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Q: Consider the compound H2S Why does the charge change between the acid and conjugate base?

A: The compound, H2S behave as an acid in it's aqueous solution. When it is dissolved in water , it…

Q: Calculate the pH of an 0.025 M solution of HCl. HCl is a strong acid.

A: Concentration of HCl solution = 0.025 M   HCl is a strong acid. Therefore, HCl completely…

Q: The pH of an aqueous solution at 25°C was found to be 6.60. The pOH of this solution is The…

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Q: What is the pH of a 0.627 M weak base solution? The Kb of the weak base is 0.000066.

A: Given :- concentration of weak base solution = 0.627 M  Kb for weak base = 0.000066  To calculate :-…

Q: What can we do to determine whether a salt forms an acidic, basic, or neutral solution when…

A: Acidic salt:  A normal salt which is formed by the neutralization of a strong acid and weak base is…

Q: Write the formula for the conjugate acid of each base.

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Q: A solution in which [H+] = 10-3 M is whereas a solution in which [H+] = 10-10 M is +. Give the pH…

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Q: What is the pH of an aqueous solution in which [H+] is 0.0025 M?

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Q: When 4.00 g of NaOH are dissolved in 100 mL of water, the pH of the solution is? [pH]

A: interpretation- To determine the pH of the solution when 4.00 g of NaOH are dissolved in 100 mL of…

Q: The pH of a basic solution is 12.77. What is [H*]?

A: The pH of a solution is mathematically expressed as: pH=-log[H+]   ............... (1) where [H+] is…

Q: solution with pH of 8.50 has a pOH of?

A: The relation between pH and pOH is given by , pH + pOH =14 pH and pOH denote the negative log of the…

Q: The pH of an aqueous solution at 25°C was found to be 8.50. The pOH of this solution is The…

A: The pH is a scale that is widely used to measure the acidity or basicity of a solution. The pH is…

Q: If the ?a of a monoprotic weak acid is 9.0×10 -6, what is the pH of a 0.39 M solution of this acid?

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Q: If the ?a of a monoprotic weak acid is 4.6×10−6, what is the pH of a 0.12 M solution of this acid?…

A: pH of a weak acid is calculated as:

Q: he pH of a half-neutralized solution is 1.86. What is the value of [H+] and Ka?

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Q: What is meant by stating a conjuagte acid and conjugate base? What can be an example of each?

A: Conjugate Acid : It is a chemical compound formed when an acid donates a proton (H+)  to a base.…

Q: The pH of water if 5 mL of 0.5 M HCl is added to total 1 L of water (2 significant figures) is…

A: Volume of water=5mL Concentration of HCL=0.5M  Volume of water=1L pH of water=?

Q: The pH of an aqueous solution at 25°C was found to be 3.80. The pOH of this solution is . The…

A: Given information, pH of aqueous solution at 25°C = 3.80 Formula used :  pH + pOH = 14 pH = -log…

Q: What is the pH of a 6.20 x 10-3 M NaOH solution? (This solution is basic, concentration is of OH-)…

A: pH is a measure of how acidic or basic is an aqueous solution. It is measured in terms of hydrogen…

Q: What is the concentration of hydroxide ion in a 0.160 M  aqueous solution of hydroxylamine, ? What…

A: Given: The concentration of the aqueous solution of hydroxylamine (NH2OH) is 0.160 M The Kb value is…

Q: What is the pH of a 6.20 x 10-3 M NaOH solution?  (This solution is basic, concentration is of OH-)

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Q: Water with a pH value (less, greater) than 7 is basic.

A: PH value: pH value is a mathematical value used in the identification of the acidic and basic nature…

Q: If the solution concentration is 1.0 x 10-4 M HCl, then the pH value is equal to ______  and the…

A: pH is the negative logarithm of Hydrogen ion concentration. It is potential of Hydrogen ion…

Q: is the salt KF acidic, basic, or neutral?

A: An acid is a substance that gives  ions in its solution whereas a basic substance gives  ions in its…

Q: If the pH of a solution is 3.3, then the pOH is and the solution is .

A: The pH of a solution is calculated from the H+ ion concentration of that solution. pH=-log [H+] The…

Q: A solution is added to water, and the H4 concentration of the water increases. Does the property…

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Q: Consider a solution of 1.34×10-3 M hydrochloric acid. What would be the hydrogen ion concentration…

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Q: .94g of sodium hydroxide is dissolved in enough water to make 620.0mL of solution at 25 degree…

A: Molecular weight of sodium hydroxide (NaOH) = 23+1+16 = 40 gm/mol  If 40 gm NaOH is present in 1000…

Q: The pH of an aqueous solution at 25°C was found to be 5.40. The pOH of this solution is M. The…

A: Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…

Q: What is the pH of a 0.14 M solution of formic acid? What is the degree of ionization of HCHO2 in…

A: The Ka of formic acid is 1.8 X 10-4  And the ionisation reaction of formic acid is  => HCOOH…

Q: Write the formula of the conjugate acid for the following base. OH−

A: Conjugate acids and bases are Bronsted-Lowry acid and base pairs, determined by which species gains…

Q: Why conjugate pairs are composed of weak acids and strong bases, and vise versa.

A: According to Bronsted-Lowry concept, the acidic and basic character of a compound can be interpreted…

Q: What is the pH and pOH of each solution given the following [OH ]? Classify each solution as acidic,…

A: Given  pOH = -log [OH-] , pH = -log [H+] and pH + pOH = 14 1) [OH-] = 10-3 M using pOH = - log [OH-]…

Q: Formic acid, HCHO2, is used to make methyl formate (a fumigant for dried fruit) and ethyl formate…

A: The dissociation constant depicts how strong or weak any acid/base is. Weak acids always possess…

Q: Calculate the pH of a 0.052

A: Since the LiOH is a strong base, it completely dissociate into ions in its solution. So the…

Q: the ?b of a weak base is 2.2×10−6, what is the pH of a 0.27 M solution of this base?

A: The given data contains, Kb =2.2×10-6Molarity =0.27 M

Q: What is the pH of 0.0137 M NaOH? Is the solution neutral, acidic, or basic? The pH is: The solution…

A: Given that,[NaOH] = 0.0137 Mfind the OH- - log [OH-] = pOHpOH = -log [0.0137] = 1.86

Q: conjugate acid of a strong base is always a weak b  strong c  neutral d amphoteric

A: Conjugate acid of weak base is a strong acid and the conjugate base of a weak acid is strong base.…

Q: When a strong acid is added to a weak base and mixed, which of the following would not be produced?…

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Q: A 0.0001 molar basic solution is 1.50 % ionized. What is the pH of the solution if its Kb= ?

A: pH of solution is defined by the number of H+ present in the solution.

Q: Calculate the pH of a 0.10 M HCN solution that is 0.0070% ionized. Group of answer choices

A: Given: Molarity of HCN       = 0.10 M Percent of ionization = 0.0070%

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.