28. 25.00 mL of a solution of a weak monoprotic acid, HX, was titrated with a 0.0640 M solution of NaOH, requiring 18.22 mL to neutralize the acid. If the Ka for the acid is 3.60*10-6, calculate the number of moles of a salt, NaX, that must be added to produce a pH of 6.00 in 150.00 mL of the original solution. You may assume that the temperature is 25 °C. It is impossible for a solution with this composition to have a pH of 6.00 0.00117 mol 0.0252 mol 0.0466 mol O 1.17 mol

Q: 0.400 M

A: A) mmoles of Acid = 60.0mL • 0.355molL-1 = 21.3mmol  B) mmles of Base = 75.0mL • 0.400molL-1 =…

Q: How is adding twice the amount of vinegar (the analyte in a titration) going to affect the amount of…

A: 1) when we add twice the amount of vinegar , the amount of NaOH will also become double . From M1V1=…

Q: A buffer solution is made that is 0.315 M in H₂S and 0.315 M in KHS. If Kal for H₂S is 1.00 x 10-7,…

A:

Q: You are asked to prepare a buffer solution with pH 5.10. If you start with a solution containing…

A: Answer: Part A) 22.6 mmol CH3COONa                 Part B) 151 ml

Q: 100.0 ml of 0.100 M acetic acid is placed in a flask and is titrated with 0.100 M sodium hydroxide .…

A: To calculate the pH in the flask after adding 50.0 mL of 0.100 M NaOH to 100.0 mL of 0.100 M acetic…

Q: When a 28.1 mL sample of a 0.423 M aqueous hydrocyanic acid solution is titrated with a 0.462 M…

A:

Q: The pKa of hypochlorous acid is 7.530. A 59.0 mL solution of 0.133 M sodium hypochlorite (NaOCI) is…

A: Given :- The pka of hypochlorous acid is 7.530. A 59.0 mL solution of 0.133 M sodium hypochlorite…

Q: A 0.805 gram sample of an unknown monoprotic acid is dissolved in 25.0 mL of water and titrated with…

A: Titration is a volumetric analysis where the unknown concentration of the compounds is carried out…

Q: 0.00+ A different student was using 50.00 mL of the same 0.1504 M pyridine solution in a titration…

A: Given,Molarity of pyridine = 0.1504 Mvolume of pyridine = 50.00 mLMolarity of HCl = 0.188 Mvolume of…

Q: Part A: You are asked to prepare a buffer solution with pH 5.20. If you start with a solution…

A: Answer:- This question is answered by using the simple concept of buffer solution in which weak acid…

Q: How many grams of sodium fluoride should be added to 40.0 mL of 0.223 M hydrofluoric acid solution…

A: A solution containing a weak acid or a weak base along with it's conjugate base or conjugate acid is…

Q: nate (Na2CO3)corresponds to the following values: 0.53 M.   (Ka for HCO3− is 5.6 ×10−11.)  Report…

A: Ka = 5.6×10-11 pKa = -log(Ka)   = -log(5.6×10-11) = 10.25 1) As it is Acidic buffer,  pH = pKa +…

Q: A buffer solution was made by mixing equal volumes of 0.20 mol/L solutions of acetic acid and sodium…

A:

Q: A student obtains a sample of 0.02500 M acetic acid (CH3COOH, 60.05 g/mole, Ka =1.8 x 10-5). 50.00…

A:

Q: Part C For 260.0 mL of a buffer solution that is 0.2922 M in CH3 CH,NH, and 0.2677 Min CH3CH2NH3CI,…

A: The buffer solution contains C2H5NH2 (weak base) and C2H5NH3Cl (salt of strong acid and weak base).…

Q: Need help calculating the initial ph of HF (weak acid). The Ka = (6.6x10^-4). I managed to calculate…

A: Given that, Initial Concentration of HF = 0.100 M Dissociation constant of acid = 6.6 x 10-4 The…

Q: Calculate the requested values to two significant figures. If you use scientific notation, use the…

A:

Q: 55.00 mL of 0.650 M benzoic acid (Ka = 6.4x10-5) is titrated by 0.600 M NaOH. Calculate the pH of…

A:

Q: The Images provided are the way they want the problem to be solved, it's weird and I'm sorry about…

A: Given: Molarity of HF=0.394 M Volume of HF (aq) taken for titration =16.3 mL  Molarity of KOH (aq)…

Q: Anisic acid (HC8H7O3) is found naturally in anise, a well-known culinary herb and flavouring agent.…

A: Given,  Molarity of HC8H7O3 = 0.100 M  Volume of HC8H7O3 = 50.0 mL = 0.050 L Molarity of KOH = ?…

Q: You need to prepare an acetate buffer of pH 5.27 from a 0.895 M acetic acid solution and a 2.71 M…

A: Let volume of KOH = V Liter  Molarity of KOH = 2.71 M  So,  Number of moles of KOH = Molarity of KOH…

Q: A buffer solution was prepared by adding 4.92 g of sodium acetate, NaCH3CO2, to 2.50 x 10^2 mL of…

A: The objective of this question is to calculate the pH of a buffer solution after adding a certain…

Q: 10.0 mL of 0.80 M HF is titrated with 0.30 M NaOH. What is the pH of the solution after 10.0 mL of…

A:

Q: 1. 0.02 mole of HCl is added to one liter of buffer containing 0.05 mole of NH,OH and 0.03 mole of…

A: Moles of NH4 OH = 0.05mol Moles of NH4 Cl =0.03 mol Moles of HCl is 0.02 mol Now,  NH4 OH + H+…

Q: A student in chemistry lab creates a buffer by making a 1.25 L solution that has 1.50 moles of…

A: Here 2.5 L of buffer solution contains 1.5 moles of NaBrO and 2.5 moles of HBrO ka= 2×10^-9. We have…

Q: A 0.15 M solution of HIO2 is being titrated with a 0.15 M solution of NaOH. 20.0 mL of the HIO2 is…

A:

Q: Lactate is an important component in some intravenous solutions. Given pKa = 3.86 for lactic acid,…

A: pH = pKa  +  log ( [ conjugate base ]/[weak acid] ) ---------(i) pKa = 3.86 ( given) HC3H5O3…

Q: What mass (in g) of sodium formate, HCOONa, must be added to 10.0 L of a 0.483 M aqueous solution of…

A: Here, we have to find the mass of sodium formate that must be added to 10.0 L of a 0.483 M aqueous…

Q: A student made a mistake while preparing an acetic acid/acetate buffer. They intended to prepare…

A:

Q: If 1. ml of 0.50 M formic acid (HCOOH) is titrated with the strong base of 0.50 M. KOH (Ka for…

A: The pH for the equivalence point : Balance chemical equation :…

Q: Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC4H,O2 with 0.100 M Sr(OH),…

A:

Q: You are asked to make a buffer to a pH of 4.00 and you have the following acids to do it with (pKa…

A: Given , The pH of buffer = 4.00

Q: Please use 3 significant figures or 3 decimal places. What is the pH of a buffer is prepared, 1.00…

A: Aqueous Solution consists of a mixture of a weak acid and its conjugate base or weak base and its…

Q: 20.0 mL of 0.075 M aqueous solution of lactic acid CH3CH(OH)COOH, a monoprotic acid, is titrated…

A: volume of NaOH at equivalence point  pH at equivalence point  pH after adding 5.0 mL of NaOH

Q: A solution is made by mixing 205 mL of 0.100 M formic acid (Ka = 1.7 x 10-4 ) and 230. mL of 0.100 M…

A: The mixture of a weak acid and its conjugate base or weak base with its conjugate acid will form a…

Q: The pH of a bicarbonate-carbonic acid buffer is 6.18. Calculate the ratio of the concentration of…

A: The ratio of [H2CO3] to that of [HCO3-] is determined by using Henderson-Hasselbalch equation.

Q: 1.0mL of 6.0M HCl is added to 100mL of a buffer that contains equal moles of acetic acid (CH3COOH,…

A: Initial pH of the buffer containing equal moles of acetic acid and sodium acetate can be given as:…

Q: 8. b) Calculate the pH of a buffer that was prepared by mixing 45 mL of 0.01M aqueous hydrocyanic…

A:

Q: with a 0.2500M solution of NaOH. The p K of butanoic acid is An analytical chemist is titrating…

A:

Q: 25 mL of a 0.0268 M solution of an unknown monoprotic acid was titrated with 0.0633 M NaOH solution.…

A: Given: Volume of monoprotic acid (assuming HA) = 25 mL = 0.025 L                            (since 1…

Q: acid is 3.75. Calculate the pH of the buffer when (a) when 40 mL 5 M HCI was added to the buffer (b)…

A: The reaction is;Volume is given as 1 L

Q: Which of the following acids (listed with Ka values) and their conjugate base should be used to form…

A: Answer: HClO2  Amongst all options, the HClO2 acid and its conjugate is superior choice for the…

Q: When a 18.3 mL sample of a 0.460 M aqueous hydrocyanic acid solution is titrated with a 0.330 M…

A: we need to calculate the pH for the above titration

Q: How many moles of sodium hypobromite, NaBrO, should be added to 1.00 L of 0.396 M hypobromous acid,…

A:

Q: When a 20.1 mL sample of a 0.367 M aqueous hydrocyanic acid solution is titrated with a 0.492 M…

A: Answer:Number of moles of any specie in the solution is always equal to its molar concentration and…

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.