What’s the PH of a 0.14M HA solution if Ka for HA is 4.0x10^-2

Q: What is the pOH of a 0.0380 M aqueous salt solution, NaX, if the Ka for HX is 0.0064

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Q: If the OH of a solution is 2.56 x 10^3 determine the H3O and the pH of the solution. Show formula.…

A: pH + pOH = 14pOH = -log10[OH-]  use this relation to find pH pH = - log10 [H+] = - log10 [H3O+]…

Q: What are the pH and pOH of a solution of 2.0 M HI, which ionizes completely?

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Q: Calculate the pH of a solution that is 0.1230.123 M HClHCl

A: To calculate pH of a solution:

Q: What is the [OH] in a solution with a pH of 9.22? (1.7 X 10 M)

A: Given that pH of solution=9.22

Q: For an aqueous solution of 0.45 M Ba(OH)2, calculate the values of the following  parameters: [H+ ],…

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Q: What is the pH of the following solutions? Identify each as acidic, basic, or neutral. a. 0.010 M…

A: If pH is greater than 7 it is basic.  If pH is less than 7 it is acidic

Q: You have a 0.0685 M solution of Ca(OH)2 what is the ph of your solution round to 2 decimal place

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Q: determine the pH of 0.251M acid HA solution. The Ka of the HA is 3.77x10^-7

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Q: Calculate the value of pOH for a solution of strong acid with an H3O+ concentration of 3.8 x 10-9 M.…

A: Given that : H3O+ = 3.8 x 10-9 M We have to calculate the pOH and identify whether the solution is…

Q: Calculate the pH of a 1.33x10-9 M solution of LiOH.

A: The reaction will be as shown below. LiOH ----> Li+ + OH-  Assuming complete reaction, we can say…

Q: Calculate the pH of an aqueous solution of 0.0740 M potassium sulfite.

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

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Q: Calculate the pH of an aqueous solution that is 0.70 M sodium hypochlorite.

A: The given compound Sodium hypochlorite (NaClO) is a strong electrolyte. So, it dissociates…

Q: What is the pH of a 0.083-M solution of CN−? Use 4.9 × 10−10 as Ka for HCN.

A: To calculate pH of 0.083 M solution of CN-Ka=4.9x10-10CN- +H2O⇌ HCN+OH-So calculate Kb for CN-…

Q: C. For the salts given below, label the pH of the resulting solution as acidic, basic or neutral. If…

A: Here is your answer

Q: Determine the pH of a 0.500 M HA solution if the Ka of HA is 4.0 x 10.

A: The ionic equation is simply: HA --------> H+ + A- now we can write the Ka formula.

Q: Determine the pH in a 0.235 M NaOH solution.

A: pH can be calculated using pOH.

Q: The pH of a solution of household ammonia, a 0.950-M solution of NH3, is 11.612. What is Kb for NH3.

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Q: Calculate the hydroxide ion concentration, [OH], for a solution with a pH of 5.1I3.

A: Given, pH of solution =5.13we are asked to calculate the concentration of [OH-]

Q: A 0.185 M solution of a weak acid (HA) has a pH of 2.95. Calculate the acid ionization constant (Ka)…

A: Given:

Q: Calculate the pH of a solution of 2.64 M HCN solution. The K₂ for HCN is 6.2 x 10-10.

A: Given : concentration of HCN solution = 2.64 M  Ka for HCN = 6.2 × 10-10  To calculate :  pH of…

Q: Calculate the pH of a solution containing 0.00177 M hypochlorous acid (HCIO) and 0.00423 M sodium…

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Q: Calculate the concentration at which a monoprotic acid with K, = 3.0 x 10 will be 1.6% ionized.

A: Dissociation constant (K) - In dissociation reaction, ratio of concentration of product (dissociated…

Q: A 0.125 M weak acid (HA) solution has a pH of 2.25. Find the acid ionization constant, Ka-

A: Given that : Initial concentration of weak acid = 0.125 M pH = 2.25 The pH can be given by : pH =…

Q: Determine the pH of a 0.500 M HA solution if the Ka of H

A: Welcome to bartleby !  Introduction :  We have to calculate pH .

Q: The PH in a 0.050 M solution of Ba(OH)2 is:

A: pH in 0.05M of Ba(OH)2 is determined as

Q: Calculate the pH of a solution that has [H 3O +] = 5.2 × 10 –7 M.

A: pH is the potential of the hydrogen which is usually used to predict how strong an acid is. The pH…

Q: A solution is made by dissolving 0.0860 moles of Ba(OH)2 in enough water to make 755 mL of solution.…

A: Given information,    0.0860 moles of Ba(OH)2    Volume of solution is 755 mL

Q: Calculate the pH and pOH for the solution with [Ca(OH)2]= 4.29x10^-5M Is the solution acidic or…

A: The value of pH can be determined by the concentration of the hydrogen ion present in the solution…

Q: What is the pH of a solution that is 2.8×10−9 M in NaOH?

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Q: What is the pH of a solution containing 0.30 M HCOOH and 0.52 M HCOO-K?

A: Weak acid is the one which undergoes partial dissociation. Formic acid (HCOOH) is a weak acid. The…

Q: Calculate the pH of a solution when 20 mL of a 0.125 M HCl are mixed with 20 mL of a 0.050 M…

A: The balanced reaction is: 2HCl + Ba(OH)2  → BaCl2 + H2O To neutralize 1 mol of Ba(OH)2, we need 2…

Q: Calculate the equilibrium concentration of the nonionized acids and all ions in a solution that is…

A: Given, concentration of HCO2H = 0.25 M concentration of HClO = 0.10 M To find: the equilibrium…

Q: What is the pH of a solution that has a hydrogen ion con- centration of 1.0 X 10 M? 46. TATI

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Q: If the ph of 0.10 M HA (weak acid) is 4.10, calculate Ka for this weak acid.

A: From given pH value the hydronium ion concentration is determined first.

Q: When 0.100 moles of NaX salt are dissolved in water to a volume of 1.00L, the pH and solution is…

A:

Q: A 0.015M solution of cyanic acid has a pH of 2.67. Calculate the ionization constant, Ka, of the…

A: Given: Concentration of Cyanic acid(HCN) solution = 0.015 M pH = 2.67

Q: The pH of a 0.20-M solution of HF is 1.92. Determine Ka for HF from these data.

A: The Bronsted-Lowry acid-base theory was purposed by Bronsted and Lowery is called Bronsted-Lowry…

Q: Calculate the pH of each of the following solutions. a. 0.12 MKNO2 b.0.45 MNaOCl c. 0.40 MNH4ClO4

A: The question is based on the concept of salt hydrolysis. we have to calculate pH of the solution.…

Q: A 1.57 M solution of a weak acid HA is found to have a pH of 2.05.     Determine the pH of a 2.00 M…

A: The concentration of hydrogen ions can be calculated as follows-

Q: A solution is made by dissolving 0.05700 moles of Ba(OH)2 in enough water to make 330.0 mL of…

A:

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

A:

Q: Calculate the pH of solutions with the following concentrations. [OH−]= 1×10−12M

A: Given, [OH-] = 1 * 10-12 M   Required,                      pH of the solution   First, have to find…

Q: What is pH of a solution consisting of 1.35 M NH3 and 2.08 M NH,NO,? K, of NH, is 5.8 x 10 10 0 9.13…

A: Given: Concentration of NH3 = 1.35 M Concentration of NH4NO3 = 2.08 M Ka for NH4+ = 5.8×10-10 We…

Q: You have a 0.125 M solution of ammonium chloride.  If the Kb of NH3 = 1.75x10-5, calculate the pH of…

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Q: The weak acid HZ has a Kₐ of 2.55X10⁻⁴.(a) Calculate the pH of 0.075 M HZ.(b) Calculate the pOH of…

A: For weak acid HZ , pKa = -logKa = -log (2.55 x 10⁻⁴) = 4 -log2.55 = 4 - 0.40 = 3.60 (a)  pH of…

Q: Calculate pH of 0.508 M solution of NaOH

A: By using the relation between pH and pOH we can solve this problem.

Q: Calculate the the pH of a solution composed of 0.20 M ammonia and 0.15 M ammonium chloride?

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Q: a 0.365g sample of HCl is dissolved in enough water to give 2.00 x 10 ^2 mL of solution. what is the…

A: pH = -log[H+] [H+] = [HCl] = Number of moles of HCl/Volume of solution (L) Number of moles of HCl =…