what is the ph of a buffer that consists of 0.86 m HBrO (ka= 2.29 x 10-9) and 0.41 M KBr

Q: Calculate the mass of sodium acetate that must be added to 2.4 L of a 0.150 M acetic acid solution…

A: Since acetic acid is monoprotic acid Hence the pH of monoprotic acid buffer is given by…

Q: You have a 0.500 L buffer solution composed of 0.47  M formic acid (HCOOH, Ka = 1.77 x 10¯4) and…

A: The acid ionization constant for acid is 1.77×10 -4.

Q: Calculate the pH of a buffer that is 0.10 M HF and 0.080 M NaF. The Ka for HF is 3.5 x 10-4.

A: pKa of the buffer solution has to be determined for calculating the pH of the solution.

Q: Calculate the pH of the buffer (2 L) that contains, 2.0 M HClO and 1.5 M NaClO. [Ka = 3.0 x 10-8]

A: Molarity of HClO = 2.0 M Volume of buffer = 2 L No of moles of HClO = Molarity of HClO * Volume of…

Q: The Kb of ammonia is 1.76x10-5. What is the pH of a buffer which is prepared by combining 50.0mL of…

A: This question can be solved on the basis of the Handerson hasselbach equation which describes the…

Q: What is the pH of a buffer that is 0.08 M NaAc and 0.1M HAc. The Ka of HAC= 1.0 x 10^-4. O2.16 O…

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: What is the molar solubility of NiS in 0.50 M NH3? The Ksp for NiŠ is 3.0 x 10-19. The K; for…

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Q: What is the pH of a buffer made from 0.190 mol of HCNO (Ka = 3.5 x 10 4) and 0.410 mol of NaCNO in…

A: Given: Ka of acid = 3.5 × 10-4 Moles of acid = 0.190 Moles of salt = 0.410 Volume of the solution =…

Q: What is the pH of the buffer that is composed of 0.10 M Na2HPO4 and 0.15 M KH2PO4? (Ka1=7.5 x 10~³,…

A: Given: Concentration of Na2HPO4 i.e. conjugate base of KH2PO4 = 0.10 M And the concentration of…

Q: Calculate the pH of a buffer system containing 0.25 M HF and 0.5 M NaF. (Ka for HF is 7.1 x 10-4)

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Q: A buffer consists of 0.25 M KHCO3 and 0.21 M K2CO3. Given that the K values for H2CO3 are, Ka1 = 4.5…

A: Given, 0.25 M KHCO3 0.21 M K2CO3 Ka1 = 4.5 x 10-7 and Ka2 = 4.7 x 10-11

Q: Kf for the complex ion Ag(NH3)2+ is 1.7 x 107. Ksp for AgCl is 1.6 x 10-10. Calculate the molar…

A: Given : The equilibrium constants for the complex formation Ag(NH3)2+, is 1.7 X 107 and the Ksp of…

Q: 5. Calculate the pH of a solution that is 0.200 M in NH3 and 0.300 M in NHẠCI. Calculate the pH…

A: Using Henderson-Hasselbalch equation: pH=pKa+logBaseAcidpOH=pKb+logAcidBase Given:- Concentration of…

Q: A buffer consists of 0.21 M H3PO4 and 0.38 M NaH2PO4. Given that the K values for H3PO4 are, Ka1 =…

A: Given that, a buffer is made by 0.21 M of H3PO4 and 0.38 M of NaH2PO4. The dissociation constant…

Q: You are given a 40.0mL sample of 0.80M CH3CH2COOH is titrated with 0.30M NaOH.  What is the pH of…

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Q: A buffer is made using 50.00 mL of 0.7000 M HA (a weak acid, Ka = 1.000 x 10-5) and 50.00 mL of…

A: GIVEN: Initial concentration of HA=0.7000 M  Initial volume of HA =50.00 mL Initial concentration of…

Q: Calculate the molar solubility of solid Ca(OH)2 (Ksp = 6.5 x 10-6) in each of the following.  Water…

A: To calculate the molar solubility of solid Ca(OH)2 in each of the following. Water A 0.125 M…

Q: A 25.00 mL sample of magnesium hydroxide solution is titrated with 0.00500 M HCI and 2 drops of…

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Q: Consider a buffer made by adding 132.8 g of NaC,H5O2 to 300.0 mL of 1.31 M HC,H5O2 (Ka = 6.3 x 10-5)…

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Q: Consider a buffer made by adding 132.8 g of NaC-H;O2 to 300.0 mL of 1.31 M HC,H;O2 (Ka = 6.3 x 10-5)…

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Q: You have a 258.3 mL sample of 1.659 M HA (Ka = 5.97⋅10−75.97⋅10-7).  Calculate the pH of the best…

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Q: An acetic acid buffer contains 0.6 M CH3COOH and 0.6 M CH3COONA. (CH3COOH has a K, 1.76 x 105.) What…

A: Given- Concentration of CH3COOH= 0.6M Concentration of CH3COONa= 0.6M Ka of CH3COOH=1.76 ×10 -5…

Q: 1. What is the pH of a buffer that contains 0.15 M CH,COOH and 0.10 M NACH,COO (K, = 1.8 x 10 )?

A: 1) Given, Concentration of CH3COOH solution = 0.15 M [CH3COOH] = 0.15 M Concentration of NaCH3COO…

Q: Calculate the molar solubility of solid Ca(OH)2 (Ksp = 6.5 x 10^-6) in 0.125 M solution of Ba(OH)2…

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Q: You find 425.0 mLof 0.350 M sodium oxalate in the lab, and you want to use it to make a buffer with…

A: Volume of sodium oxalate = 425 mL or 0.425 L Molarity of sodium oxalate = 0.350 M Moles of sodium…

Q: Calculate the pH of a buffer that is 0.030 M acetic acid and 0.010 M sodium acetate.  The Ka for…

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Q: Calculate the pH of a buffer system containing 0.25 M HF and 0.5 M NaF. (Ka for HF is 7.1 x 10-4).

A: The acid ionization constant for HF  is 7.1×10 -4. pKa = -log Ka = -log (7.1×10-4)=3.1

Q: Which of the following salts has the highest molar solubility in pure water? 1 2 3 4 5 O O O 1 3 4 5…

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Q: What is the pH of a buffer that is 0.76 M in HF and 0.98 M in NaF? Ka = 7.1 x 10-4

A: pH = pKa + log [salt]/[acid] pKa = -logKa

Q: Calculate the molar solubility of Cd(OH)2, Ksp = 5.9 x 10-11.

A: Given: Ksp = 5.9 x 10-11 To find: the molar solubility of Cd(OH)2

Q: What is the pH of the buffer that is composed of 0.10 M Na2HPO4 and 0.15 M KH2PO4? (Ka1=7.5 x 103,…

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Q: Calculate the pH change that takes place when a 150-mL portion of a) 0.0800 M NaOH and b) 0.0800 M…

A: Solution - ∆pH by adding NaOH = 0.05 ∆pH by adding HCl = 0.04 Buffer capacity ( NaOH ) = 0.48…

Q: What is the pH of the buffer 0.10 M Na2HPO4/0.15 M KH2PO4? Ka = 6.17 x 10-8

A: The objective of the question  is to calculate the pH of the buffer solution where the buffer…

Q: What is the pH of a buffer that contains 0.20 M CH 3COOH and 0.15 M NaCH 3COO?

A: Whenever the concentrations of the acid as well as its conjugate base, or the base and its…

Q: What is the component concentration ration, [Pr]/[HPr], of a buffer that has a pH of 5.44 (Ka of HPr…

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Q: 1. A buffer is prepared containing 1.00 molar Acetic Acid and 1.00 molar Sodium Acetate. What is its…

A: A buffer solution is made by the mixture of a weak acid with its conjugate base or by the mixture of…

Q: What will be the pH change when 20.0 mL of 0.100 M NaOH is added to 80.0 mL of a buffer solution…

A: According to the mole concept, in terms of mass, the amount of substance in moles is equal to the…

Q: Calculate the pH of the 0.30 M NH3/ 0.36 M NH4C1 buffer system. What is the pH after addition of 20…

A: A buffer is a solution which resist change in pH and obtained when a weak acid and the salt of its…

Q: A general chemistry student performs a titration with 28.4 mL of 0.294 M weak acid solution with a…

A: Introduction The details and data about the H+ ions (hydrogen ions) are derived by deriving any…

Q: What is the molar solubility of Ca(OH)2? Ksp = 8.0 x 10-6

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Q: Consider a buffer made by adding 42.3 g of (CH3)2NH2I to 250.0 mL of 1.42 M (CH:)»NH (Kb = 5.4 x 10…

A: pH is a scale which is used to determine the acidity or basicity of a solution. pH = pKa + log…

Q: How many grams of solid sodium fluoride should be added to 0.500 L of a 9.49x10-2 M hydrofluoric…

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Q: Consider the titration of a 60.0 mL of 0.355 M weak acid HA (Ka = 4.2 x 10⁻⁶) with 0.400 M KOH.…

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Q: Consider a buffer made by adding 52.3 g of (CH3),NH,l to 250.0 mL of 1.42 M (CH3)2NH (Kb = 5.4 x…

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Q: What is the pH of a buffer that consists of 0.412 M methylamine CH3NH2 and 0.219 M methylammonium…

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Q: What is the pH of a buffer composed of 0.45 M C5H10NH and 0.65 M [C5H10NH2]Cl?

A: Formula for calculating pOH of a solution consisting of a weak base and its salt with a strong acid:…

Q: How many grams of sodium hypochlorite, NaCIO, need to be added to 227 mL of a 0.185 M solution of…

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.