What is the pH of a 40.0 mL solution that is 0.11 M in CN and 0.25 M in HCN? The K, for HCN is 4.9 x 109. pH =

Q: The K, of a certain base is 4.4x107. What is the pH of a 0.30-M solution of this base?

A: Hello. Since your question has multiple questions, we will solve the first question for you. If you…

Q: The Kb of C6H5NH3+ is 3.98x10-10 What is its Ka? What is the [H3O+] concentration in a solution…

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Q: Find the OH- and pH of 0.25g of Ba(OH)2 dissolved in enough water to make 0.655 L  solution?

A: Given, the amount of Ba(OH)2 =0.25 gramvolume of solution =0.655 Lmolar mass of Ba(OH)2 =171.34…

Q: What is [OH-] in a solution of 0.125 m ch3nh2 and 0.130 m ch3nh3cl?

A: Buffers are the solutions containing a mixture of weak acid and its conjugate base or a mixture of…

Q: If the K, of a weak base is 7.2 × 10-6, what is the pH of a 0.33 M solution of this base? pH =

A: in this question given data is  α=KaC   ka×kb=10-14C=0.33MPH=-logH+ Apply the value given formula,…

Q: An unknown weak base with a concentration of 0.0910 M has a pH of 10.70. What is the Kb of this…

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Q: What is the pH of a solution that is 2.7×10-9 M in NaOH

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Q: Which solution has the higher pH, a 0.001 M solution of NaOH or a 0.001 Msolution of Ba(OH)2?

A: The simplification is as follows:

Q: What is the pH in a solution consisting of Ba(OH)2 6.17x10-8M.

A:

Q: An unknown weak base with a concentration of 0.170 M has a pH of 9.15. What is the Kb of this base?

A: Solution:       Weak bases on dissociation show partial ionization. This means that an equilibrium…

Q: A solution of sodium acetate (NaCH3COO0 has a pH of9.70. What is the molarity of the solution?

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Q: If the K of a weak base is 7.0 × 10-6, what is the pH of a 0.37 M solution of this base? pH :

A: We make an ICE table then equilibrium constant expression is written ,since we have weak acid so we…

Q: An aqueous solution has [H+] = 1.0 x 10-4 M. What is the [OH−] for this solution?

A: Given, [H+] = 1 × 10-4 M We have to find [OH-] .

Q: An unknown weak base with a concentration of 0.0910 M has a pH of 11.90. What is the Kb of this…

A: Given: Concentration of base = 0.0910 M And pH of solution = 11.90  Since pOH = 14 - pH => pOH =…

Q: pH and pOH

A: MMoles of NaOH = M × V     = 5.0×10-3 × 350  = 1.75 mmol After adding water, Concentration of  NaOH…

Q: If a 5.6 L solution has a pH of 3.6, what will the pH be if the volume is increased to 7.2 L?

A: Given:PH of solution-1 = 3.6V1 = 5.6 L.V2 = 7.2 L

Q: A solution of sodium cyanide, NaCN, has a pH of 11.20. How many grams of NaCN are in 835 mL of a…

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Q: Please help me, double check your answers as previous tutors got it wrong.

A: pH is the potential of the hydrogen or the power of the hydrogen. It basically explains how acidic…

Q: What quantity of moles of glucose (C₆H₁₂O₆) in 0.500 L of a 0.400 M solutions?     The pH of a basic…

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Q: What volume of a 15.0% by mass NaOH solution, which has a density of 1.116 g/mL, should be used to…

A: Relationship between pH and pOH. Molarity is the number of moles of solute dissolved in per litre…

Q: what is the pH of solution made by adding 22 g of KoH into water and diluting to 250.0 ml?

A: The mass of KOH is 22g. It is dissolved in water to form of 0.250L of solution. The number of moles…

Q: If 29.7 mL of 0.205 M KOH is required to completely neutralize 25.0 mL of a CH;OOH solution, what is…

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Q: If the K, of a weak base is 2.7 x 10, what is the pH of a 0.30 M solution of this base?

A: Solution Ph may be a live of however acidic or basic is AN solution.It is measured in terms of…

Q: The pain reliever codeine is a weak base with a K, equal to 1.6x10-6. What is the pH of a 0.05 M…

A: pH of a solution is defined as the negative  logarithm of H+ ion concentration. Given codeine…

Q: An unknown weak base with a concentration of 0.0910 M has a pH of 10.80. What is the Kb of this…

A: Welcome to bartleby!  Introduction :  We have to calculate Kb of the base .

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: A certain weak base has a Kb of 8.40×10−7. What concentration of this base will produce a pH of…

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Q: A chemist wants to make 20.00 L of a 0.25 M HCl solution. A) How many milliliters of a 11 M HCl…

A: A) Volume of 11M HCl required = 454.55 mL B) pH = 0.6021

Q: If the K, of a weak base is 1.7 × 10-6, what is the pH of a 0.18 M solution of this base? pH =

A: pH of a substance represents the strength of an acid or base. If the pH is small, it is a strong…

Q: If the K of a weak base is 8.0 × 10-6, what is the pH of a 0.48 M solution of this base? pH

A: Weak base dissociated less in aqueous solutions

Q: Calculate [H3O+] in a solution that has [OH−] = 6.7×10−2 M at 25°C. Is the solution neutral, acidic,…

A: Given,  [OH−] = 6.7×10−2 M

Q: What is the pH of a solution that has an [OH-] of a 7.3 x 10^-9 M?

A: Given, Concentration of the OH- ion = [OH-] = 7.3 x 10-9 M pH of the solution = ? The formula used…

Q: What is the pH of a 40.0 mL solution that is 0.13 M in CN¯ and 0.27 M in HCN? The K, for HCN is 4.9…

A: Interpretation-  To determine the pH of the 40mL of solution that is 0.13M in CN- and 0.27M in HCN .…

Q: A certain base has a Kb of 7.8 × 10-6 . What concentration of the base will produce a pH of 11.32?

A: Fristly we calculate the concentration of OH- from the pH : pOH = 14-pH  = 14-11.32 =2.68…

Q: If the K of a weak base is 5.6 × 10-6, what is the pH of a 0.40 M solution of this base? pH

A: Given:  Kb = 5.6×10-6 Concentration = 0.40 M Since, the value of Kb and concentration of base is…

Q: Determine the pH, OH -, H3O+ and ph for a solution made by dissolving 121 mg of HCl in 555 mL of…

A: First the reaction between HCl and water is determined.

Q: A solution of hydroiodic acid has a concentration of 2.00x10-2 M. What is the pH of this solution?…

A: Given: Concentration of hydroiodic acid i.e. HI = 2.00 × 10-2 M.

Q: A student measures the temperature of an NaOH solution to be 40°C. The student then measures the pH…

A: PH is defined as the negative log of the concentration of H+ ion. PH = -logH+   POH is defined as…

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: You have a 7.4x10-4M Sr(OH)2 solution. What is the pH of this solution?

A: First of all we will calculate pOH then pH

Q: An unknown weak base with a concentration of 0.0910 M has a pH of 11.20. What is the Kb of this…

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Q: Are these solutions acidic, basic, or neutral? Then on the section below, categorize HCI and HC2H3O2…

A: We have to categorize HCI and HC2H3O2 as either weak or strong acids as follows in step 2:

Q: What is the pH of a 7.5 × 10-3 M OH solution? pH = [? ]

A: The question is about calculating the pH of the given solution with the concentration of Hydroxide…

Q: A certain weak base has a Kb of 8.60×10−7M. What concentration of this base will produce a pH of…

A:

Q: The pH of 0.55 M aqueous solution ammonia HN3 at 25.0 degree C is 11.50. What is the value of Kb for…

A: NOTE : You have given HN3 instead of NH3. Since the pH is in basic zone, hence the specie will be…

Q: An unknown weak base with a concentration of 0.170 M has a pH of 9.37. What is the Kb of this base?

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

Q: An aqueous NaOH solution has a hydroxide concentration equal to 0.02 mol/L. The NaOH concentration…

A: Given: The hydroxide concentration is 0.02 mol/L.

Q: A solution has [H3O+] = 1.20 x 10-4 M. What is the pH of the solution?

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.