Suppose you have just added 50.0 ml of a solution containing 0.0400 moles of weak acid HA to 500.0 ml of 0.6000 M NaOH. What is the final pH? The Ka of HA is 1.77 × 10-5.

Q: H+] = 2.575 x 10^-5 M; calculate pH

A: As we know pH is given by pH = -log[H+]

Q: A weak acid, HA, has a p?apKa of 4.5424.542. If a solution of this acid has a pH of 4.4944.494, what…

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Q: What is the pH of an acetic acid solution (HC2H3O2) with concentration 0f 0.100 M. Ka=1.75 x 10-5 A.…

A: An ICE table is constructed to determine the equilibrium concentration of H3O+ as follows,

Q: A 0.17 M solution of a weak acid has a pH of 2.85. What is the ka of the weak acid?

A: Given: concentration of weak acid=0.17M              pH of weak acid=2.85 To calculate: Ka of weak…

Q: What is the pH (aq., 25 oC) of 30.00 mL of a 0.250 M HBr solution that has had 15.00 mL of 0.125 M…

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Q: Calculate the pH of a 0.27 M solution of HCO2H (formic acid, Ka = 1.8 x 10–4).

A: PH = - log [H +] Formic acid weak acid  Ka =dissociation constant

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: Which of the following solutions will have the lowest pH value? A.) 0.10 M HNO3 B.) 0.03 M H2SO4…

A: Given acids: A.) 0.10 M HNO3 B.) 0.03 M H2SO4 C.) 1.0 M HCN (Ka = 4 X 10-10) D.) 2.0 M…

Q: NH3 is a weak base (?b=1.8×10−5) and so the salt NH4Cl acts as a weak acid.   What is the pH of a…

A: There are two types of bases/acids. One is strong base/acid which is completely dissociable in into…

Q: solution is prepared at 25°C that is initially 0.41M in chloroacetic acid (HCH2ClCO2) , a weak acid…

A: Given,  Concentration of Acid = 0.41 M Concentration of Salt = 0.0821 M Ka = 1.3 ×10-3 pKa = 2.89 As…

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: Determine the pH of 80 mL of a 0.30 M solution of acetic acid when 0, 40 mL, 80 mL and 100 mL  of…

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Q: For each of the following cases, decide whether the pH is less than 7, equal to 7, or greater than…

A: the correct option are as follows:

Q: For a solution of an aqueous hypochlorous acid solution, the Ka is 5.0 x 10-8 and [HOCI] is 0.050M.…

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Q: Given that the Ka of a monoprotic acid HA is 3.20 x 10-7 , and the acid HA concentration is 0.751 M,…

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Q: What is the concentration of an aqueous HI solution that has a pH of 2.26?     1.82 x 10-2 M…

A: Given that, pH = 2.26  Then, [HI] = ?

Q: A typical aspirin tablet contains 325 mg acetylsalicylic acid (HC 9 H 7 O4). Calculate the pH of a…

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Q: Calculate the pH of 0.30 M methylamine, CH3NH2, which has a Kb of 4.4 x 10-4.

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Q: 2) Determine the pH of a solution by adding 0.23 mole formic acid and 0.17 mole of sodium formate in…

A: Henderson Hasselbalch equation is given by, pH=-log(Ka)+log[salt][acid] where Ka is the acid…

Q: An unknown weak acid with a concentration of 0.085 M has a pH of 1.80. What is the Ka of the weak…

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Q: calculate the pH a solution prepared by adding 20.0 mL of 0.020 M NaOH to 0.10 M Na3AsO4.

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Q: A 0.250 M solution of a weak base has a pH of 9.91. Calculate the Kb of this base. Kb = ______ x…

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Q: We put 0.628 mol of a weak acid, HA, and 12.7 g of NaOH in enough water to produce 1.00 L of…

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Q: should have a lower pH. Explain your choice. a) 0.10M HCl or 0.20M HCl b) 0.10M HCl or 0.10M HF c)…

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Q: A 1.0 × 10 -2  M aqueous solution of Ca(OH) 2 at 25.0 °C has a pH of? 12.30     12.00     2.0 ×…

A: Answer:- This question is answered by using the simp[le concept of calculation of pH of the solution…

Q: ^-3

A: Question 01:  We know that the conjugate acid base pair differs by a single electron.  Therefore the…

Q: Calculate the pH of a solution that is 1.9 x 10^-2 M Ba(OH)2.

A: pH of a solution is equal to the negative logarithm of hydronium ion concentration while pOH is…

Q: Calculate the pH of the following solutions: (a) 0.0500 M NaOH (b) 0.0500 M sodium acetate (c)…

A: A)   0.05 M  NaOH    As NaOH is a strong base, it will dissociate completey.   NaOH (aq) → Na+ (aq)…

Q: 2. Calculate the pH of a solution when 10.00 mL of 0.1000 M NaOH is added to 20.00 mL of 0.1000 M…

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Q: What is the pH of a solution with 10.2mL 0.10M CH3COOH and 0.15mL 1.0M HCl ? Ka = 1.8x10^-5

A: pH is the negative logarithm of the hydrogen ion concentration. It is a measure of acidity or…

Q: Which of the solutions listed below has the lowest pH?    A.  Pure H2O  B.  2.5 x 10-5 M HNO3  C.…

A: Lowest pH mean stronger acid and higher pH mean stronger base .

Q: A solution whose pH is equal to 4.0 has a hydrogen ion concentration of _____.  (A)1 x 104 M (B)1 x…

A: The pH of a substance is given by, pH = -log[H+]

Q: Calculate the pH of a solution prepared by dissolving 0.0775 mol acetic acid (HCOOH) and 0.0460 mol…

A: Given-> Moles of HCOOH = 0.0775 mole Moles of HCOONa = 0.0460 mole Volume = 1 L Ka = 1.77 × 10-4…

Q: The pH of an aqueous solution of sulfurous acid, H2SO3, that has a concentration of 0.60 mol/L and…

A: The solution is as follows:

Q: After dissolving 0.35 g of magnesium hydroxide in 135 mL of water, how many mL of a 1 L hydrochloric…

A: M= n / V(in L)   where   n = moles of solute (Mg(OH)2) = mass / molar mass = 0.35 g / 58 g/mol   =…

Q: A 0.10 M sample of a weak acid has a Ka of 4.0 x 10 −5. What is the pH of the weak acid? Between 3…

A: Let HA be the weak acid. It ionizes in the solution as follows:                               HA…

Q: Calculate the pH of a 0.020 M solution of phenylacetic acid, C6H5CH2COOH. What will be the pH if the…

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Q: Arrange the following solution from lowest pH to highest pH: a) 0.20 M CH₃COOH (Ka = 1.8 x 10⁻⁵),…

A: (a) First of all First of all the ICE table has to be drawn for the dissociation of acid as:…

Q: Codeine (C 18H 21NO 3, 299.36 g/mol) is a weak base. Suppose a 2.00 g pain tablet containing 30.0 mg…

A: Given that, Molar mass of codeine = 299.36 g/mol Mass of codeine in 2.0 g pain tablet = 30 mg = 0.03…

Q: Suppose 5.00 g of propanoic acid (HC3H5O2) is dissolved in enough water to yield 100.0 mL of…

A: Molar mass of propanoic acid = 3×12+6×1+2×16=74g/mol Number of moles = massmolar…

Q: HIO3 has a ka of  0.16. What is the pH of a 0.600 M HIO3 solution? (use successive approximations)

A: The strength of an acid depends on the extent of its dissociation in water. Strong acids dissociate…

Q: a. 35 mL of 0.15 M H₂SO4 is mixed with 35 mL of 0.30 M NaOH O The pH of the solution is less than 7.…

A: pH is the measure of acidity or basicity of a solution. A solution with pH higher than 7 is basic…

Q: the lab you prepare a 0.50 M solution of a weak acid "HA" . You measure that the pH of this solution…

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Q: What is the pH of a solution that is 0.80M benzoic acid and 0.20 M sodium benzoate ?  Ka HC6H5O2 =…

A: Record the given data, Concentration of benzoic acid is 0.80 M Concentration of sodium benzoate is…

Q: alculate pH of each solution and determine if solution is acidic, basic, or neutral. [OH-] = 1.9 x…

A: To calculate the pH of each solution and to determine whether it is acidic, basic or neutral. [OH-]…

Q: Calculate the pH of a 0.10M weak acid, HA, whose Ka is 1.8 X 10

A: Given that: Concentration of weak acid,(HA) = 0.10M Ka = 1.8×10-5 Weak acid partially dissociates…

Q: What will be the pH of a solution of a weak acid (HB), of concentration 0.15 M (Ka = 1.8x10-5

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Q: Calculate the pH, when the following solutions are added to 100. mL 0.10 M HClO solution: The Ka of…

A: Given :-  Molarity of HClO solution = 0.10 M = 0.10 mol/L  Ka of HClO = 3.0 x 10-8…

Q: weak acid, HA, has a p?a of 4.331. If a solution of this acid has a pH of 4.458, what percentage of…

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Q: 1. Which has the lowest pH? Explain why. 0.10M HCl or 0.20M HCl

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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.