A buffer solution contains 0.53 mol of hydrosulfuric acid (H2S) and 0.10 mol of sodium hydrogen sulfide (NaHS) in 8.70 L. The Ka of hydrosulfuric acid (H2S) is Ka = 9.5e-08. (a) What is the pH of this buffer? pH = ____

Q: A buffer solution is made that is 0.314 M in HF and 0.314 M in KF. If Ka for HF is 7.20 x 10-4, what…

A:

Q: When a 18.5 mL sample of a 0.327 M aqueous hydrofluoric acid solution is titrated with a 0.457 M…

A: we have to calculate the pH of the solution

Q: A 5.296 g sample of a solid, weak, monoprotic acid is used to make a 100.0 mL solution. 30.00 mL of…

A:

Q: 29. The acid HA has an ionization constant of 10-5, If 50 ml 0.1N HA is diluted to 200 ml and…

A: Ka (HA) = 10-5  pKa = -logKa        = -log ( 10-5 )        = 5Initial Normality of HA =M1 = 0.1…

Q: When a 22.7 mL sample of a 0.343 aqueous hypochlorous acid solution is titrated with a 0.385 M…

A: Given ,

Q: You prepare 500 mL buffer solution that contains 0.50 moles monoprtic weak acid (HA) and 0.30 moles…

A: Number of moles of weak acid = 0.50 mol Number of moles of conjugate base = 0.30 mol Ratio of…

Q: When a 16.8 mL sample of a 0.459 M aqueous hydrofluoric acid solution is titrated with a 0.459 M…

A:

Q: A buffer solution is 0.412 M in H₂S and 0.236 M in NaHS. If Ka1 for H₂S is 1.0 × 10-7, what is the…

A:

Q: Which of the following acids is best to use to prepare a buffer with a pH of 4.5? НОC HАОСООН, Ка 3…

A:

Q: A buffer is made by dissolving 10.5 g of sodium dihydrogen phosphate, NaH2PO4 and 12.0 g disodium…

A:

Q: A buffer is prepared by using 0.20 mole of C6H5COOH and 0.40 mole of C6H5COO- in 1.00 liter of…

A: The objective of this question is to determine whether the buffering capacity of a solution,…

Q: b) A buffer solution is prepared by adding 40.0 g of sodium acetate CH;COONA to 500 mL of a 0.200 M…

A: Given: Mass of CH3COONa =40.0g Molar mass of CH3COONa =82.03 g/mol Volume of solution =500ml=0.5 L…

Q: Calculate the pH of a buffer solution containing 0.716 mol HA weak acid and 0.607 mol A- in 239.9 mL…

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

Q: A chemistry graduate student is given 300. mL of a 1.20M nitrous acid (HNO2) solution. Nitrous acid…

A: Answer:Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: 8) If 100.0 mL of 0.250 M HBr is titrated with 0.150 M KOH answer the following questions. a) What…

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

Q: A buffer solution contains 0.31 mol of phenol (HC6H5O) and 0.85 mol of sodium phenoxide (NaC6H5O) in…

A: Given:  Moles of phenol (HC6H5O) = 0.31 mol Moles of sodium phenoxide (NaC6H5O) = 0.85 moles Volume…

Q: A buffer solution is made such that the initial concentrations of lactic acid (HC3H5O3) and the…

A:

Q: An buffer is prepared by combining 1.61 moles of HX solution with 0.28 moles NaX and diluting to a…

A: Given :- number of moles of HX = 1.61 mol  Number of moles of NaX = 0.28 mol  Total volume = 1 L  Ka…

Q: What is the final pH when 0.032 mol of NaOH is added to 0.422 L of a solution containing 0.428M…

A: pH = pKa + log[C3H5O2-]/[HC3H5O2] Number of mol = Molarity x Volume (L)

Q: 1. Consider the reaction HBr + KOH --> KBr + H2O One performed the titration of HBr (0.130 M, 25.00…

A:

Q: Name: NetID: 8. A titration is carried out where 50.0 mL of 0.300 M HF is titrated with a 0.190 M…

A:

Q: A buffer solution is made that is 0.462 M in HCIO and 0.462 M in KCIO. If K₂ for HClO is 3.50 ×…

A: Given -> [HClO] = 0.462 M  [KClO] = 0.462 M  Ka(HClO) = 3.50 × 10-8  Mole of HI = 0.102 mole…

Q: A solution NH3 that contains 78 mL of 0.043 M ammonia, NH 3, is titrated with 0.083 M HCI. The K₁ of…

A: Given,Molarity of NH3 = 0.043 Mvolume of NH3 = 78 mLMolarity of HCl = 0.083 MKb of NH3 = 1.8 x 10-5

Q: A 1.00 L solution contains 0.372 M HA (Ka = 2.93⋅10−62.93⋅10-6) and 0.741 M NaA.   What is the pH…

A: Here we are required to find the pH of the solution.

Q: Consider a buffer solution that is 0.47 M HCN and 0.47 M NaCN. (Ka(HCN) = 4.9 × 10−10) Calculate…

A: After addition of 0.20 mol of NaOH the [ HCN ] = ( 0.47 - 0.20 ) = 0.27 M And [ NaCN ] = ( 0.47 +…

Q: 100.0 mL of 0.120 M ammonium hydroxide (Kb = 1.75 x 10-5); Kw = 1.00 x 10-14) is to be titrated with…

A:

Q: A 100.0 mL buffer solution is constructed using 0.035 M HX, a weak acid, and 0.045 M NaX. Ka. HX =…

A:

Q: What’s the PH=

A: Given that, 2.05 g of sodium acetate is dissolved in 85.0 mL of 0.10 M of acetic acid solution. The…

Q: A solid hydroxide, with the formula M(OH)3, is dissolve to make a saturated solution. If the pH of…

A: Solubility indicates the maximum amount of a substance that can be dissolved in a solvent at a given…

Q: What is the pH of the resulting buffer solution when 25mls of 0.10 M NaH is added to 25mls of 0.200…

A: pH of the buffer solution is calculated by using Henderson equation, it is,

Q: Buffer capacity is a measure of a buffer solution's resistance to changes in pH as strong acid or…

A: Henderson-Hasselbalch equation, Is an equation which shows the relationship between the pH and pOH…

Q: a) Calculate the pH of the solution formed when 100 cm³ of 0.100 mol dm³ H₂SO, is added to 50 cm³ of…

A: Pls repost your question ( 5) .

Q: What are the molar concentrations of acetic acid (CH,COOH) and sodium acetate (CH,COONA) in an…

A: Buffer solution: buffer solution  is an aqueous solution consisting of a mixture of a weak acid(HA)…

Q: 1. Consider Ammonia, NH3, with Kb= 1.8x10-5 (a) What is the pH of a buffer solution prepared by…

A: (a).  Number of moles of NH4Cl = Given mass of NH4Cl in g / Gram molar mass of NH4Cl = 13.36 g /…

Q: A buffer solution is 0.405 M in H2CO3 and 0.397 M in KHCO3. If Kal for H2CO3 is 4.2 × 107, what is…

A: The objective of the question is to calculate the .

Q: How to calculate the pH of a buffer solution 1) Calculate the pH of a solution prepared by…

A:

Q: Consider the titration of 50.00 mL of 0.100 M benzoic acid (HC7H5O2, Ka = 6.3 × 10−5) (aq) with…

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

Q: Suppose you need to prepare a buffer system with a pH = 5.30 in the laboratory. The available acids…

A:

Q: 4) What is the pH of a buffer solution, prepared by mixing of 75 mL 0.1 M CH3COOH solution and 150…

A: In this question we have to tell the PH of the buffer solution.

Q: Aspirin (C 9H 8O 4) is a weak monoprotic acid (K a = 3.3 x 10-4). You are analyzing a sample for a…

A: The question is based on the concept of pH of the solution.  It is defined as a negative logarithm…

Q: A buffer solution contains 0.77 mol of hydrosulfuric acid (H2S) and 0.43 mol of sodium hydrogen…

A: Here the reaction is, H2S(aq) + H2O(l) ⇌HS- (aq) + H3O+(aq) Here, Ka= 9.5×10-8 From Henderson…

Q: What is the pH of a buffer solution that is 0.214 M in ammonia and 0.390 M in ammonium chloride…

A: First calculate Ka value for ammonia and use it to calculate the pH of the buffer solution.

Q: A solution prepared by mixing 1.73 of propionic acid (HC3H5O2) and 0.53 g of NaOH in water (Ka…

A:

Q: A buffer solution is made such that the initial concentrations of lactic acid (HC3H5O3) and the…

A: We have to find pH of given buffer on addition of KOH

Q: Moly Cule is titrating 0.2 M of a strong base (NaOH) into 100 ml of a solution of 0.1M weak acid…

A: Given: Molarity of NaOH  = 0.2 M Volume of solution = 100 mL Molarity of HAc     = 0.1 M Ka for HAc…

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.