Ka for HCN is 6.2 x 10-10. The pH of an aqueous solution of 0.10M of NaCN is?

Q: Calculate the pH of a solution containing 0.00261 M hypochlorous acid (HCIO) and 0.00256 M sodium…

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Q: If we have a solution of weak acid HA (Ka = 1,00 * 10-6) and at pH 4,00. How much water needs to be…

A: Hey, as the volume of weak acid is not given in the question, I consider it as 25 mL in order to…

Q: A) 0.0956 g ammonium chloride, and made 50.0 mL of solution, what would the initial pH of this…

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

Q: Temperature-Dependence of Kw: The autoionization of water is an endothermic reaction. According to…

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Q: Calculate the [OH-] and pH of a mixture formed by adding 50.0 mL of 0.0.20 M HCl to 150 mL of 0.010…

A: Given : Concentration of HCl = 0.020 M                                                     (Assuming…

Q: A chemist makes four successive 1:10 dilutions of 1.0X10⁻⁵ M HCl. Calculate the pH of the original…

A: The pH of a solution is the negative of logarithm of the concentration of hydrogen ions in the…

Q: What concentration of barium hydroxide is needed to give an aqueous solution with a pH of 12.800?…

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Q: A certain weak base has a K, of 7.20 x 10-7, What concentration of this base will produce a pH of…

A: Base dissociation constant Kb is utilized to determine the basic nature of a solution. It refers to…

Q: How many grams of ammonium chloride, NH4Cl, would have to be added to exactly 500 mL of 0.10 M NH3…

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Q: What is the pH of a solution that is 0.12 M in HOCl and 0.20 M in NaOCl?  Ka of HOCl is 3.5 x 10-8…

A: Given, 0.12 M in HOCl and 0.20 M in NaOCl

Q: Consider an aqueous solution that is 0.050 M in H2Se (Ka = 1.29 x 104) and 0.075 M in NaHSe. Out of…

A: The acid ionization constant for acid is 1.29×10 -4.

Q: The Kw for water at 0 °C is 0.12 × 10-14 M². Calculate the pH of a neutral aqueous solution at 0 °C.…

A: In this question, we have to calculate the pH of a Neutral solution at 0°C when Kw for water at 0°C…

Q: When answering this problem, report the answer with the appropriate number of significant figures.…

A: When a solution is diluted by adding water, concentration changes.

Q: Q3// Grams of Sodium Formate required to add to 40oml of o.1M Formic acid to make the pH of solution…

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Q: The Kw for water at 0 °C is 0.12 × 10-14 M². Calculate the pH of a neutral aqueous solution at 0 °C.…

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Q: The pH of an aqueous solution at 25°C was found to be 9.80. The pOH of this solution is The…

A: 1) Given that : pH of the solution = 9.80 pOH of the solution is, pH + pOH = 14 pOH = 14 - pH = 14 -…

Q: 3 > Calculate the pH of each solution at 25 °C. 5 М НСI 1.0 × 10 M HCI pH = 0.01 M HNO, pH= 3. 1.0 x…

A: Hello. Since your question has multiple sub-parts, we will solve first three sub-parts for you. If…

Q: You are given 30 Calculate the values of both pH and pOH of the following solutions: pOH pH 0.020M…

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Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0176 M solution. The pH of the…

A: given values are - initial concentration of monoprotic acid = 0.0176 M pH = 2.47  Ka = ?

Q: Given that Ka for HCN is 6.2×10−10, calculate Kb for CN-. Express your answer to two significant…

A: 1- First question, Calculate the value of Kb for weak base CN- ion :  We know that, Kb × Ka = Kw  Kb…

Q: What is the pH of a solution with a hydroxide ion (OH-) concentration of 10-10M?

A: pH is related to pOH by the following expression: pH + pOH = 14  ⋯⋯⋯⋯(1) Also pOH is related to the…

Q: Determine the pH of an aqueous solution of KOH at 25oC if it is 5.00 x 10-8 M in KOH. Hint: Consider…

A: From given

Q: Write the reaction that occurs and calculate the pH. a) 15.0mLof0.10MNaOHisaddedto5.0mLof0.15MHCl…

A: Since, To get pH, [H+] or [H3O+] should be calculated.

Q: A certain weak base has a ?b of 7.30×10^−7. What concentration of this base will produce a pH of…

A: pH of the base is 10.25. The sum of pH and pOH of a solution is equal to 14.

Q: A chemist dissolves 592. mg of pure barium hydroxide in enough water to make up 160. mL of solution.…

A: At 25 oC, the solubility of barium hydroxide, Ba(OH)2 is approximately 4.70 g / 100 mL water.  Since…

Q: Q3// Grams of Sodium Formate required to add to 40oml of o.1M Formic acid to make the pH of solution…

A: Henderson-Hasselbalch equation The equation that is used to find the pH of a buffer solution is…

Q: Calculate the pH of the solutions about with 1.3x10^-6 M: a. sodium hydroxide solution b. barium…

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Q: Calculate the pH of an aqueous solution that is ( Ka(HCN) = 6.20 × 10 10-10) a. 0.870 M in HCN. pH =…

A: We know that  HCN is a weak acid it doesn't dissociate completely. The dissociation reaction will be…

Q: Find the [H+] and pH of a solution of 0.1 Molar HCN and 0.1 Molar of NaCN.  Ka = 2.0 x 10‒4.

A: Given: The concentration of HCN (hydrogen cyanide) is 0.1 M The concentration of NaCN (sodium…

Q: The pOH of an aqueous solution at 25°C was found to be 9.20. The pH of this solution is . The…

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Q: Consider an aqueous solution that is 0.050 M in H2Se (Ka = 1.29 x 10-4) and 0.075 M in NaHSe.  Out…

A: Given,  0.050 M in H2Se 0.075 M in NaHSe

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 pH of a solution of 1.0 × 10-9 M NaOH (include 1 digit after the decimal in your…

A: The pH of any compound can be calculated on the basis of the concentration of hydronium ions present…

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: A 30.0 mL aliquot of a solution is 0.25 M HCl . If 0.1 M NaOH is to be added to this solution,…

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Q: 07-13: The diprotic acid Hal. has Kor 1.4 x 10% and Ka 1.2 x 10-¹0 97-Calculate the molarity of H*…

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Q: a) Consider CH3COONH4: What is the solution pH if this compound is dissolved in it? Given the Ka of…

A: Given,  Acid dissociation constant of CH3COOH = Ka = 1.8 x 10-5  Acid dissociation constant of NH4+…

Q: pH

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Q: Calculate the pH of an aqueous solution that is 0.35 M NH3 and 0.15 M NHẠNO3 given that the K of NH3…

A: Given solution which have NH3 ( a weak base ) and NH4NO3 ( conjugate salt of NH3) , would form a…

Q: he hydronium ion concentration in an aqueous solution at 25°C is 2.6×10-2 M. The hydroxide ion…

A: pH is defined as the negative logarithm of hydrogen ions. The acidic, basic r neutral nature of…

Q: The Ka for H2S is 9.1x10^-8. Calculate the pH of a .15 M solution of H2S in water

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Q: The pOH of an aqueous solution at 25°C was found to be 13.00. The pH of this solution is The…

A: The given p (OH) at 25°C = 13.00 At 25°C, pH + p (OH) = 14 The pH = 14 – 13 = 1 Therefore, pH = 1.

Q: Q3// Grams of Sodium Formate required to add to 40oml of o.1M Formic acid to make the pH of solution…

A: Given that: molarity of formic acid = 0.1 M Volume of solution = 400 mL Ka = 1.74×10-4 M.wt of…

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0120 M solution. The pH of the…

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Q: Consider the following data on some weak acids and weak bases: name acid acetic acid hydrocyanic…

A: Here we have to determine the increasing order pH of the following salt solution.  pH of salt…

Q: A certain weak base has a K, of 8.20 x 107. What concentration of this basc will produce a pH of…

A: Given, pH= 10.29 Kb = 8.20*10-7

Q: Calculate the pH of a 0.0100 M solution of 10.00mL of carbonic acid and 10.00mL of 0.0050 M sodium…

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Q: A chemist dissolves 461. mg of pure barium hydroxide in enough water to make up 180. mL of solution.…

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Q: Consider the following data on some weak acids and weak bases: name acetic acid hydrocyanic acid 0.1…

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Q: The Ka for a weak monoprotic acid is 3.3 x 10-11. The pH of a 2.5M aqueous solution of this acid is

A: Weak acids undergo partial dissociation and at certain stage it develops equilibrium with the…

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.