A 25.00-mL solution containing NaOH, Na2CO3, and NaHCO3 alone or in compatible combination was titrated with 0.0998 M HCl using phenolphthalein as indicator. The solution turned colourless after addition of 25.65 mL of HCl. Methyl orange was then added to the solution and an additional 6.95 mL of the acid was needed to change the colour of the indicator. Identify the components in the mixture and calculate the concentration of each in milligrams per millilitre of solution.

Q: A buffer is made using 100.0 mL of 0.200 M CH3 CH2 COOH (propanoic acid) and 100.0 mL of 0.100 M…

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Q: Calculate the volume in milliliters of 0.368 M KOH necessary to titrate 0.0209 moles of acetic acid…

A: Given : Concentration of KOH = 0.368 M Moles of HOAc = 0.0209 mol

Q: Discuss the titration curve (variation of pH with respect to addition of titrant) with suitable…

A: A question based on pH titration curve, which is to be accomplished.

Q: The weak acid acetic acid, CH3COOH(aq), is titrated with strong base potassium hydroxide, KOH(aq).…

A: At Equivalence point acid and base both titrated with each other and strong base complete…

Q: 0.3 g of a weak acid was dissolved in 75 mL water. Phenolphthalein indicator was added. 0.1 M…

A: Answer: In this question Henderson-Hasslebalch equation won't come in use because at the end point,…

Q: Strong base is dissolved in 535 ml of 0.400 M weak acid (K = 3.41 x 10-5) to make a buffer with a pH…

A: Given,  Ka = 3.41 X 10-5 [HA]initial = 0.4 , Volume = 535 ml pH of buffer solution = 3.94

Q: buffer of pH = 7.5 is desired. Which two of the following compounds should be dissolved in water in…

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: In which case medium in Equivalent point is expected to be neutral: titration of H2SO4 by KOH…

A: The titration of strong acid with strong base gives a neutral solution at equivalence point. The…

Q: buffer was made by combining 84.29 mL of 0.20 M acetic acid (pKa = 4.756) and 107.98 mL of 0.15 M…

A: A buffer is a solution which resist any change in pH on adding a small amount of acid or base . it…

Q: A buffered solution was prepared by dissolving 6.85g of sodium formate (NaHCOO in 250.0mL (16) of a…

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Q: What is the pH of a buffer that is 0.41 M HCN(aq) and 0.87 M NaCN(aq)? The Ka of HCN is 6.2 x 10-10.…

A: A numerical problem based on Henderson equation, which is to be accomplished.

Q: Determine the pH of the buffer solution produced by the reaction of 5 mL 0.1 M KOH and 30ml 0.1…

A: Given that : Concentration of CH3COOH = 0.1M Volume of CH3COOH = 30mL = 30×10-3L Concentration of…

Q: Phosphate buffers are present in biological systems such as the blood plasma. If a buffer solution…

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Q: The titration of 100.mL of 0.100 M NH3 (in the flask) with 0.200 M HCL (in the burette) was carried…

A: In the given scenario, we conduct a titration experiment between a weak base, ammonia (NH3), and a…

Q: A buffer solution is prepared by dissolving 1.50g each of benzoic acid (MM=122.1, Ka=6.3 x 10^-5),…

A: Given,  Mass of benzoic acid (HC7H5O2) = 1.50g Molar mass of benzoic acid =122.1g/mol Mass of sodium…

Q: A purified protein is in a 100. mM HEPES buffer pH 7.3 with 500. mM sodium chloride (NaCl). A 25.0…

A: Given that: pH = 7.3 Concentration of HEPES with NaCl = 100 mM  Concentration of NaCl in HEPES…

Q: (iii) How much lime is required to precipitate the hardness in 2.5 litres of this tap water? How…

A: The detailed answers with explanations for the above questions can be found below step

Q: Calculate the pH during the titration of 30.00 mL of 0.1000 M ammonia with 0.1000 M HCl(aq) after…

A: Given: Molarity of ammonia = 0.100 M Volume of ammonia = 30.00 mL Volume of HCl= 12.46 mL Molarity…

Q: What is the difference between alkalinity and buffering capacity?

A: The ability of a solution to resist pH fluctuations by either absorbing or desorbing H+ and OH- ions…

Q: A buffer solution is prepared by dissolving 1.00 g of sodium acetate (CH3COONa) into 100.00 mL of a…

A: Given: The concentration of acetic acid is 0.100M. The volume of acetic acid is 100 mL. The…

Q: A saturated solution of magenusium hydroxide is prepared and the excess solid magneusium hydroxide…

A: Given that : The volume of magnesium hydroxide = 25 mL Concentration of HCl = 0.00053 M Volume =…

Q: NH4

A: Given: Ammonia buffer solution: M1 =  0.25 M [NH4+] M2   = 0.22 M [NH3] pKa of NH4+ = 9.24

Q: c. Use the pH curve, and the information show in the table above, to select the most appropriate…

A: In an acid-base titration, a known volume of either the acid or the base (of unknown concentration)…

Q: An ammonia buffer solution contains 0.20 M NH4+NH4+ and 0.21 M NH3NH3 . The pKa of ammonium is…

A: A buffer is a solution which resists any change in pH on adding a small amount of acid or base.It is…

Q: Calculate the pH of a titration mixture when 25.36 mL of 0.081 M NaOH has been added to a 50.00 mL…

A: In this question we have to tell the PH of the mixture of the given solution. This solution create a…

Q: A buffer is composed of 0.200 M (CH3)2NH (Kb = 5.9 × 10–4) and 0.250 M (CH3)2NH2NO3. What is the pH…

A: pKb  = - log Kb            =  - log (5.90  * 10-4 )          = 3.23pKa = 14-pKb       = 14- 3.23…

Q: Suppose you performed a titration of a weak acid and you found that the equivalence point occurred…

A: Given that,  The volume of NaOH required to reach the equivalence point = 19.51 mL And Acid is a…

Q: Which of the following acids is the best choice to prepare a buffer at pH 9.4 when paired with their…

A: The value of pH for titration of weak acid with strong base is calculated by Henderson-Hasselbalch…

Q: The primary buffer in the blood is carbonate-bicarbonate buffer. If the pKa is 6.1 and the pH is set…

A: GIVEN DATA:-Buffer is Carbonate (CO32-) and Bicarbonate (HCO3-).                          pH=7.4…

Q: A 65.0 mL solution of 0.158 M potassium alaninate ( H, NC, H, CO, K) is titrated with 0.158 M HCI.…

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Q: Indicator Measurement Colour of Indicator phenol red pOH = 6.8     Indicator Measurement Colour of…

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Q: Calculate the pH during the titration of 20.00 mL of 0.1000 M dimethylamine, (CH3)2NH(aq), with…

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Q: the strong acid hydrobromide acid, HBr(aq) is titrated with strong base sodium hydroxide, NaOH(aq).…

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Q: What is the pH of a buffer solution if you dissolve 300 ml of 1.65M Formic Acid (HCO2H) and 250 ml…

A: Given -> Volume of formic acid = 300 ml  Molarity of formic acid  = 1.65 M = M1 Volume of sodium…

Q: The pKa of acetic acid is 4.74. What is the pH of a buffer solution that is prepared from 0.010 M…

A: Buffer solution have tendency to resist pH change on addition of small amount of strong acid or…

Q: A buffer solution is prepared by mixing together 29.00 mL of 0.15 mol L1 HA (a monoprotic weak acid…

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Q: 2.80 g of sodium acetate, CH3COONa was dissolved in 150.0 mL of water, H2O. A solution of 0.025 M…

A: The pH of the mixed solution can be calculated by Handerson-Hasselbach equation.  pH = pKa + log…

Q: Lactobacillus bulgaricus is the main bacterium used in the production of yogurt and requires an…

A: The available weak acids are: (i): Benzoic acid, HC6H5COO, pKa1 = 4.19 (ii): Carbonic acid, H2CO3,…

Q: An aqueous buffer solution of volume 100 cm3 consists of 0.20 M CH3COOH and 0.20 M NaCH3CO2.…

A: a) Calculation of pH of the solution: Thus pH of the solution in 3 significant figures is 4.75

Q: A student has a sea water sample which contains Ca2 ions . Describe briefly how he will determine…

A: To determine the concentration of calcium ions, we have to perform titration with EDTA solution. In…

Q: Click the "draw structure" button to launch the drawing utility. Draw the product formed in the…

A: Three-membered rings formed by two carbon and one oxygen atoms are known as epoxide rings. The…