Calculate the Kb of a 0.26 M solution of X OH that has a p H of 12.9.

Q: : Calculate the hydroxide ion concentration of a 0.0750M H3 solution. The Kb is 1.75 x 104. Use the…

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Q: Use the "Square of Death" to determine the following for the solution in problem 6 where pH =…

A: We have find out the answer.

Q: How many gram of ammonia should be added to 500mL of 1M ammonium chloride to give a pH 9? Ka…

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Q: Calculate the concentration of OH- ions in a 1.4 x 10-3 M HCl solution.

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Q: Calculate the Kb of a 0.41 M solution of X OH that has a p H of 12.1

A: pH of solution is equal to the negative logarithm of hydronium ion concentration. pH=-log(H3O+). Kb…

Q: aqueous solutions will have a pH of 2.00 at 25 °C? (Kw = 1.01 × 10–14) 0.020 M HNO3

A: As we know,  Acidic solution has pH less than 7. Basic solution has pH greater than 7 . pH =…

Q: A sample of Ca(OH)2 with a mass of 0.151 g is dissolved in water so that the volume of the solution…

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Q: Selected information about five solutions, each at 24oC, is given in each part.  Fill in the blanks…

A: If concentration of hydroxide ion is greater then hydronium ion concentration then solution is basic…

Q: Find the [H3O+][H3O+] concentration of a 0.290 M M  acetic acid solution. (The value of KaKa for…

A: Given, the concentration of acetic acid =0.290 Mand Ka for  acetic acid =1.8×10-5 we are asked to…

Q: What is the pOH of pure water at 40 oC? ( K w at 40 oC = 2.87  × 10 –14)

A: Given: Kw at 40oC = 2.87 × 10 –14 The reaction is as follows,

Q: Calculate [H30*] for a 0.0038 M Ba(OH)2 solution. What is the answer please

A: The molarity of the barium hydroxide solution is 0.0038 M. The barium hydroxide is a strong…

Q: Which 0.10 M solution will have the largest concentration of hydroxide ion?     NH3 (Kb of NH3 =…

A: Which 0.10 M solution will have the largest concentration of hydroxide ion, it is to be determined.…

Q: Calculate the pH of a 5.0 x 10-8 M HCl solution. Report your answer to the hundredths place. pH =…

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Q: Calculate [H, o*] for a 2.63 x 10-3 M HBr solution. [H,O*] = M Calculate [H, o*] for a 1.00 x 10-2 M…

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Q: Calculate the pH and the pOH of these solutions:     (a) 0.257 M HBr pH =   pOH =     (b) 0.332 M…

A: Since you have posted a question with multiple sub-parts, we will solve first two subparts for you.…

Q: What is the pOH of a solution that contains 5.3 x 10-5 M HCl at 25°C?

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Q: Q4. Hydrochloric acid solution with 0.015 M, if you take 50 ml from it and diluted by water to 150…

A: Given : Initial concentration of hydrochloric acid i.e HCl = 0.015 M Initial volume of HCl solution…

Q: Find the pH of a solution 1.4 M in NH3. For NH3 K-1.8x10-5. Report your answer to two decimal…

A: Given is Kb = 1.8 × 10–5 We will use the method of finding Kb by equilibrium concentration

Q: Below are some properties associated with acid solutions and some properties associated with base…

A: Acids are sour in taste. Whereas bases are bitter in taste.

Q: How much volume (in Liters) is required to neutralize 126 mL of 0.55M H3PO4 if we use a 3M Ca(OH)2…

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Q: Ammonia has a pKb=4.75. Work out how much ammonia is in the form of NH4+ in a 0.01 Molar solution at…

A: Ammonia in water exists as: NH3+H2O↔NH4OH→NH4++OH-

Q: In EACH of the pairs of aqueous solutions listed below, CIRCLE which of the two is the MORE BASIC…

A: a) Given: NaNO3 and NaNO2

Q: Which 0.20 M solution will have the largest concentration of hydroxide ion?       NH3 (Kb of NH3 =…

A: 1- In this question, we will see which species give largest hydroxide ion concentration.  You can…

Q: Calculate [A-] and [A2-]of a 0.050 M solution of diprotic acid, H2A, with K1 = 8.5 x 10-5 and K2 =…

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Q: . What is the value for the dissociation constant of the base? 1.459x10^-5 1.897x10^-4 1.799x10^-5…

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Q: Find the pHpH of a 0.291 MM KClOKClO solution. (The KaKa of hypochlorous acid, HClOHClO, is…

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Q: In a 0.100M solution of lactic acid (HC3H5O3), %dissociation is 3.70%. Calculate the Ka.

A: Given data  % dissociation = 3.70 % Concentration ( initial ) = 0.100 M  lactic acid (HC3H5O3)…

Q: The kw for water is 5.5 x 10-14 at 50oC.  What is the pH of a neutral aqueous solution at 50oC?…

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Q: Consider the following data on some weak acids and weak bases: acid base K. K, name formula name…

A: Applying concept of pH we can determine order of pH of given Salt.

Q: Calculate [H,O*] for a 8.92 × 10–3 M HBr solution. [H,O*] = M Calculate [H,O+] for a 1.20 x 10-2 M…

A: Given,  (A).  [HBr] = 8.92 x 10-3 M  [H3O+] = ? (B).  [KOH] = 1.20 x 10-2 M  [H3O+] = ?

Q: Which of the following solutions has a p

A: Salt hydrolysis : the process in which cation (or) anion (or) both of a salt reacts with water to…

Q: Rank the following solutions according to their acidity: Rank [4,0*] Solution 1 = 10° M %D Solution…

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Q: Which of these statements are true for a neutral, aqueous solution at 25 °C? O (H*] = [OH"] pH =…

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Q: Determine the pHpH for the following solutions: [OH−]=5.8×10−4M[OH−]=5.8×10−4M Express your answer…

A: pH is equal to negative logarithm of hydrogen ions

Q: Calculate [H,O*] for a 5.04 x 10-3 M HBr solution. [H,O*] = M Calculate [H,O*] for a 1.60 × 10-2 M…

A:

Q: A solution has [H+] = 4.0 x 10-3 M. The [OH"] in this solution is %3D 4.0 x 1011 1.0 x 10 14M 4.0 x…

A: Given data,[H+]=4.0×10-3M

Q: Calculate the pH when 1.03 g of NaClO (FW = 74.44 g/mol) is added to 44.4 mL of 0.50 M HClO. Ignore…

A: Answer: In this question we have to calculate the pH of the buffer made of HClO and NaClO.

Q: Calculate (H,O*] for a 5.19 x 10-3 M HBr solution. [H,O*) = Calculate (H,O*] for a 1.60 x 10-2 M KOH…

A: Hydrogen bromide is a strong acid and the strong acid dissociates completely in an aqueous solution.

Q: Consider the following five solutions: Solution A:  [OH-] = 1.66 x 10-5 MSolution B: pH =…

A: p H of solution A and B can be calculated using the equation given below:

Q: What is the pH of a 0.712 M weak acid solution that has a Ka = 4.5 x 10-9?

A: Weak acids dissociate partially. So we have to calculate degree of dissociation first and then pH.

Q: U16HW Question 8 Homework • Unanswered Fill in the Blanks Type your answers in all of the blanks and…

A: pH is a scale to measure a substance acidic or alkaline in nature . It's value range 0 to 14 . For…

Q: 6. In Group C, do all four compounds appear to be molecular, ionic, or molecular acids? Based on…

A: Group 'C' means the 14th group element. In the 14th group carbon (C), silicon (Si), germanium (Ge),…

Q: Calculate the hydroxide ion concentration of a 0.0750M NH3 solution. The Kb is 1.75 x 104. Use the…

A: Answer: When Ammonia will be added in the water, following reaction will take place:…

Q: Consider the following data on some weak acids and weak bases: acid base K, K, name formula name…

A: Given tables are : And  Complete the table in order of increasing pH value = ?

Q: When the concentration of H3O+ is 6.5 x 10-7 the solution is an acid, a base or neutral.  Choose the…

A: pH of a solution can be calculated by taking the logarithm of the concentration of hydronium ions in…

Q: Calculate the [H*] of 5.8 x 10-5 M magnesium hydroxide solution. O [H*] = 3.4X10-11 O [H*] =…

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Q: Putting 10g of H2SO3 in 95mL of water will give an acid with what concentration

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Q: The acid dissociation K, of benzoic acid (C,H5CO,H) is 6.3 × 10 °. Calculate the pH of a 1.0M…

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Q: 4. What is the pH of a 2.15 x 10-3 M oxalic acid (H2C2O4). The Ka of oxalic acid is 6.4 x 10-5.

A: pH = - log [H3O+]  Oxalic acid is a weak acid and do not undergo complete ionisation in solution.…

Q: What is the pOH of a solution that contains 1.2 x 10-5 M HCl at 25°C?

A: Given,  Concentration of HCl = [HCl] = 1.2 x 10-5 M  pOH of the solution = ?

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.