use henderson hasselbalch equation to calculate the ph of buffer solution that is 0.50 m in bh3 and 0.2m in nh4cl for ammonia pkb=4.75

Q: A 50.0 mL sample of 0.100 M NH, is titrated with 0.100 M HBr. What is the most likely pH of the…

A: Answer :- 2.041  pH = 2.041…

Q: (a) Calculate the pH of a buffer solution containing 0.40 mole of KF and 0.50 mol of HF in 1.50…

A: pH of buffer solution is calculated using Henderson–Hasselbalch equation, amount of strong acid HCl…

Q: Calculate the pH of a solution that is 0.45 M CH3COOH and 0.75 M NaCH3COO. Sodium acetate/acetic…

A: Buffer is a solution which consists of a weak acid and it's conjugate base or weak base and it's…

Q: A buffer solution contains 0.50 mol of hydrazoic acid (HN3) and 0.62 mol of sodium hydrazoate (NaN3)…

A: This problem is solved on basis of Handerson-Hassalbalch equation

Q: important values if needed for Which of the following aqueous solutions are good buffer systems?…

A: Given: Some of the following solutions which can act as a buffer systems  To find: which of the…

Q: Which is the best solution to buffer at pH = 10.50?           (A) A buffer solution containing 0.25…

A: Henderson-Hasselbalch equation The equation that is used to calculate the pH of a buffer solution is…

Q: Ammonia is a convenient buffer system in the slightly basic range. (a) What is the pH of a buffer…

A:

Q: of arsenous acid (H3AsO3) and 0.87 mol of sodium dihydrogen arsenite (NaH2AsO3) in 7.30 L. The Ka of…

A:

Q: 3. If 50.00 mL of 1.00 M HC,H,O, (K, = 1.8 x 105) is titrated with 1.00 M NAOH. What is the pH of…

A: In this question , we are given a weak acid ( acetic acid ) and it is titrated with a strong base (…

Q: you want to separate Ni2+ and Mn2+ by precipitating the corresponding sulphides from each other.…

A: Given dataKsp (NiS): 10-21,Ksp (MnS): 10-15,Ksp (H2S): 10- 20 ,Saturation concentration of H2S in…

Q: A buffer solution is made that is 0.411 M in CH3COOH and 0.411 M in CH3CO0NA. (1) If K, for CH3COOH…

A: Answer:- This question is answered by suing the simple concept of calculation of pH of a solution…

Q: An aqueous solution is prepared to be 0.248 M in sodium acetylsalicylate and 0.123 M in benzoic acid…

A: Given: Concentration of benzoic acid, C6H5COOH=0.123 M Concentration of sodium acetylsalicylate,…

Q: A buffer solution is made that is 0.320 M in H2CO3 and 0.320 M in KHCO3. If Kal for H2 CO3 is 4.20 ×…

A: Solution: pH of acidic buffer = pka + log(KHCO3/H2CO3) pka1 of H2CO3 = -logka1                 =…

Q: buffer solution contains 0.40 mol of arsenous acid (H3AsO3) and 0.87 mol of sodium dihydrogen…

A:

Q: A buffer solution is made that is 0.414 M in HClO and 0.414 M in KCIO. If Ka for HCIO is 3.50 ×…

A: The objective of this question us to calculate the pH value of the given reaction.

Q: A chemistry graduate student is given 100. mL of a 1.40M chlorous acid (HC1O,) solution. Chlorous…

A:

Q: A chemistry graduate student is glven 125. mL of a 1.10M pyridine (C,H,N) solution. Pyridine is a…

A: The given data contains, Volume = 125 ml. Molarity = 1.10 M.

Q: 11) Choose the acid below that would make the most effective buffer for a solution to maintain a pH…

A: The solution is given below -

Q: A 75.0 mL sample of 0.0200 M HBrO4 is titrated with 0.0400 M RbOH solution. Calculate the pH after…

A: Given -  Volume of HBrO4 = 75.0 mL Molarity of HBrO4 = 0.0200 M Molarity of RbOH = 0.0400 M

Q: Calculate the pH at the equivalence point in titrating 0.057 M solutions of each of the following…

A: Concentration of NaOH = 0.079 MEquivalence Point: It is a point at which, equivalent quantities of…

Q: A chemlstry graduate student Is glven 300. mL of a 1.50M trimethylamine ((CH, N solutlon.…

A: The pH of the solution is the power of protons in the solution. While pOH is related to the basicity…

Q: Calculate the pH of a buffer solution that is 0.74 M in NH3 and 0.74 M in NH4Cl. For NH3, pKb =…

A: PH= 14-pKb- log[NH4+]/[NH3]

Q: Calculate the pH of a bicarbonate buffer that is composed of a solution that is 0.5 M sodium…

A: To calculate the pH of a bicarbonate buffer solution, you can use the Henderson-Hasselbalch…

Q: Calculate pH for a weak base/strong acid titration. Determine the pH during the titration of 35.9 mL…

A: “Since you have posted a question with multiple sub-parts, we will solve the first three sub-parts…

Q: Determine [Zn2 ], [CN–], and [HCN] in a saturated solution of Zn(CN)2 with a fixed pH of 3.610. The…

A: Given:The pH of the solution is 3.610 The solubility product (Ksp) of Zn(CN)2 is .The Ka of HCN is .

Q: Calculate the pH at the equlvalence point in titrating 0.096 M Solutions ol ed (a) hydrobromic acid…

A: Since, pH represents the concentration of hydrogen ion in the given solution. pH=-logH+

Q: A 250-mL buffer solution contains 0.0510 mole of KH2PO4 and 0.0875 mole of K2HPO4. (a) Calculate…

A:

Q: 0.20 moles of CuSO4 are added to 1L of NH3 1.20M solution. Calculate the concentration of Cu2+ in…

A: Data given: Moles of copper sulfate = 0.20 mol Molar concentration of ammonia = 1.20 M Volume of…

Q: What [NH3] needs to be added to 0.0010M NH4Cl to obtain a buffer solution with pH of a 7.3?

A: pH of buffer solution is calculated by using Henderson Hassel balch equation

Q: A buffer solution contains 0.289 M KH2PO4 and 0.399 M K2HPO4. If 0.0485 moles of hydroiodic acid…

A: To calculate the pH of the resulting solution when 0.0485 moles of hydroiodic acid are added to 250…

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.