Q: If a water has a carbonate alkalinity of 120.00 mg/L as the ion and a pH of 10.30, what is the…
A:
Q: Calculate the mass (in g) of sodium benzoate (NaC7HsO2) that would obtain a buffer with a pH of 4.30…
A: Henderson Hasselbalch equation for buffers: pH = pKa + log [salt]/[acid] Here acid is benzoic acid…
Q: The pH of a 0.5L HNO2-NO2 buffer solution was determined to be 4.23. The solution was mixed with 5g…
A: Given, pH of buffer solution = 4.23 pKa = 4.35 Volume of buffer solution = 0.5 L weight of HNO2 = 5…
Q: A buffer is created by adding 0.321 moles of bromoacetic acid (pKa = 2.902) and 0.555 moles of…
A: Given that : Moles of acid (bromoacetic acid) = 0.321 moles Moles of salt (sodium bromoacetate) =…
Q: A buffer solution is prepared by dissolving 1.0 mole of the weak acid CH3COOH (pKa = 4.74) and 1.0…
A: The initial pH of the buffer can be calculated as follows-
Q: Determine the pH of the buffer solution produced by the reaction of 5 mL 0.1 M KOH and 30 mL 0.1 M…
A: Chemical equation: CH3COOH (aq) +KOH(aq) ⇌ CH3COOK (aq) + H2O (l)
Q: What mass of potassium lactate in g must be added to 0.85 L of a 0.41 mol L1 solution of lactic acid…
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Q: What volume of 0.12M HCN and 0.13M CN- would be required prepare 500mL of pH =9 buffer? The pKa of…
A: Given data,Molarity of HCN=0.12MVolume of CN-=0.13MVolume of buffer=500mLpH=9pKa=9.21
Q: A 1.00 L phosphate buffer solution that contains 0.1270 moles of dihydrogen phosphate (H2PO4) and…
A:
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: A buffer solution is made that is 0.357 M in HCN and 0.357 M in KCN. If Ka for HCN is 4.00x10^-10 ,…
A: Given : Concentration of weak acid HCN = 0.357 M Concentration of conjugate base salt of weak acid…
Q: A buffer solution with a pH of 3.86 is prepared with 0.50 M formic acid and M sodium formate. The K,…
A: The formula of pH of a buffer solution is: pH=pKa+log[Salt][Acid]
Q: You prepare 250.0 mL of a buffer solution containing 0.550mol of acid and 0.450mol of its conjugate…
A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid
Q: Determine the pH of the buffer solution produced by the reaction of 5mL 0.1 M KOH and 30 mL 0.1 M…
A: Given-> Volume of KOH = 5 ml Molarity of KOH = 0.1 M Volume of CH3COOH = 30 ml Molarity of…
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: A buffer solution is prepared by taking 0.400 moles of acetic acid (pKa = 4.76) and 0.250 moles of…
A: The Henderson Hasselbalch equation for acidic buffer solution is given as :
Q: Many chemical reactions are carried out in the presence of buffers. Use the Henderson-Hasselbalch…
A: Range for the target pH of a buffer solution that would favor pH stabilization using Henderson…
Q: A solution is made by dissolving 0.1283 g of the acid form of the buffer TRIS (molecular mass =…
A: According to the mole concept, in terms of mass, the amount of substance in moles is equal to the…
Q: A Phosphate Buffer NaH2PO4 - K2HPO4 with a final volume of 500. mL, concentration of 0.10M with a…
A: A buffer is a solution which resist any change in pH on adding a small amount of acid or base . it…
Q: Suppose there is 1.00 L of an aqueous buffer containing 60.0 mmol of formic acid (pKa=3.74) and 40.0…
A: Weak acid are those acid which does not dissociate completely in aqueous solution and weak base are…
Q: A chemist titrates 210.0 mL of a 0.1055M hypochlorous acid (HCIO) solution with 0.3543M KOH solution…
A: Reaction between HClO and KOH is shown below: HClO(aq)+KOH(aq)→KOCl(aq)+H2O(l) According to reaction…
Q: A buffer solution is composed of 5.00 mol of acid and 1.75 mol of the conjugate base. If the pKa of…
A:
Q: How many grams of sodium acetate (82.03 g/mol) must be added to 1.00 L of 0.50 M solution of acetic…
A:
Q: Using the concentrations 0.100M and 0.1766M, and the pKa of 3.752, what is the theoretical pH of a…
A: pKa = 3.752
Q: A 38.05 mL aliquot of weak base that has a concentration of 0.577 M will be titrated with 0.39 M…
A: Concentration of weak base = 0.577 M = 0.577 mol/L Volume of weak base solution = 38.05 ml = 38.05…
Q: 2. There is a phosphate buffer with 0.1 M of NaH₂PO4 0.1 M of Na₂HPO4. Calculate pH of buffer…
A: A buffer solution is a combination of two solutions - a weak acid solution and the salt of its…
Q: A buffer solution is made that is 0.307 M in H2CO3 and 0.307 M in KHCO3 . If Ka for H2CO3 is…
A: Given concentration of H2CO3 is 0.307 M and concentration of KHCO3 is 0.307 M. Acid dissociation…
Q: What is the pH of a buffer that is .1 Molar in H2CO3 and 1M in NaHCO3?
A:
Q: A buffer solution is prepared by mixing 0.35 mol L1 solution of citric acid, C5H¬O5COOH, and 0.40…
A: Given: Concentration of citric acid (Assuming HA) = 0.35 M Concentration of sodium citrate (Assuming…
Q: A substance X was shown to be a weak acid with a single pKa value of 3.00. Using the, a 1.0-L buffer…
A:
Q: Calculate the pH of a buffer system containing 2.0 M CH3COOH and 2.0 M CH3COOK.The pKa of CH3COOH is…
A: Concentration of CH3COOH=2.0M Concentration of CH3COOH=2.0M pKa of CH3COOH=4.74
Q: A student needs to prepare a buffer solution with a pH of 5.26. Assuming a pKa of 4.73, how many mL…
A: A buffer solution is the one which is formed by mixing “a weak acid with the solution of the salt of…
Q: 3. The maximum buffering capacity is nearest to the pka of the buffer. Explain why?
A:
Q: Acetic acid and its conjugate base acetate can form an acid-base buffer. The pKa of acetic acid is…
A: Acid dissociation constant is the physical constant used to determine the strength of an acid. It is…
Q: A solution of the primary standard potassium hydrogen phthalate (KHP), KHC,H,O,, was prepared by…
A: Given data,Mass of KHP=0.4877gVolume of water=50mLVolume of KOH=19.26mL
Q: The colour of Phenolphthalein indicator in basic medium is O colourless O Blood red O Pink O Red
A: Phenolphthalein is an indicator used in acid - base titration. Phenolphthalein changes its colour…
Q: You make a Buffer using a Weak acid (HA) with a pKa of 7.95 and its Conjugate Base Salt (NaA). You…
A: pH = pKa + log{[A-]/[HA]} = 7.95 + log(0.100/0.500) = 7.95 - 0.698 = 7.25
Q: The Ka values for nitrous acid (HNO2) and hypochlorous (HClO) acid are 4.5 x10-4and 3.0 x10-8,…
A: The pKa values of HNO2 and HClO is calculated below. The pKa of HClO is closer to the required pH…
Q: A buffer solution is to be made wherein the pH of the acetic acid (pKa = 4.74) buffer is 5.08. If…
A:
Q: Acetic acid and its conjugate base acetate can form an acid-base buffer. The pKa of acetic acid is…
A: A solution which resists change in pH when a small amount of acid or base is added to it is known as…
Q: 7. solution was observed to be 5.45, exactly halfway to its equivalent point. What is the Ka and pKa…
A:
Q: . What cations may be present in a pale blue solution that turns deep blue and forms a white…
A: solution- Cu2+ ion solution has pale blue solution and the reaction. the reaction between copper…
Q: Calculate the pH of a buffer solution containing 0.92 M NaF and 0.44 M HE. The pKa of HF is 3.14.
A: Given that : Concentration of NaF = 0.92M Concentration of HF = 0.44M pKa = 3.14 pH of the buffer…
Q: A buffer is created by adding 0.125 moles of hypobromous acid (HOBr, pKa = 8.65) and 0.475 moles of…
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Q: The Ka values for nitrous acid (HNO2) and hypochlorous (HClO) acid are 4.5 * 10-4 and 3.0 * 10-8,…
A: Given data: The Ka values for nitrous acid are 4.5 ×10-4. The Ka values for hypochlorous acid…
Q: A buffer solution is prepared by taking 0.250 moles of acetic acid (pKa = 4.76) and 0.400 moles of…
A: From the Henderson-Hasselbalch equation:
Q: pH of a buffer solution prepared by mixing 20 mL of 1 M NH4OH and 40 mL of 2 M NH4CI will be (pKp of…
A: Given data Buffer solution has 20 mL of 1 M NH4OH40 mL of 2 M NH4Cl pKb = 4.7 for NH4OH…
Q: Calculate the pH of a buffer solution obtained by dissolving 11.011.0 g of KH2PO4(s and 29.0g of…
A:
Q: A buffer is made up of equal volumes of 0.1 M weak acid (AH) and 0.1 M conjugate base (A minus). The…
A: Given :- concentration of weak acid i. e. [HA] = 0.1 M Concentration of conjugate base i. e. [A-]…
Q: A maximum of 0.50 g of CuX(100 g/mol) will dissolve in 100 mL of a 1.0M ammonia buffer (total…
A: The solubility product constant or the equilibrium constant is a measure of the extent to which the…
500ml of a 0.1M sodium phosphate buffer with pka of 7.21is diluted. Calculate the pH of of the buffer when it is diluted with water
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- A buffer solution is prepared from an unknown weak acid (HA) and its conjugate salt (NaA). If 500.00 ml of this buffer solution contains 0.025 moles of HA and 0.066 moles NaA, and has a measured pH of 4.61, what is the pKa of the unknown weak acid?Calculate the pH of a bicarbonate buffer that is composed of a solution that is 0.5 M sodium carbonate and 0.05 M carbonic acid. The pK is 6.10.A solution was found to have a PH of 6.3 with the acid 100x in excess of it conjugate base. What is the pKa of the solution would it be considered a buffer
- The pH of a buffer solution containing 0.35 M acetic acid and 0.39 M sodium acetate where the pKa of acetic acid is 4.75 is_________________Using the concentrations 0.100M and 0.1766M, and the pKa of 3.752, what is the theoretical pH of a buffer solution?Consider a buffer solution containing an acid with a pKa of 2.3 and an acid concentration that is one fourth the concentration of the conjugate base. What is the pH of the solution?
- What molar ratio of salt to acid would be required to prepare a buffer solution with a pH of 5.9? The pK a of the acid is 5.7.Suppose that a 1000 mL buffer (pH=5) solution will be prepared using 2.6g C6H5COOH (its Ka is 6x10-5) and 2.6g NaC6H5COOH in H2O. How much (in g) of the component of the buffer should be added in the 1000mL buffer so that its pH will be 3?A buffer is created by adding 0.321 moles of bromoacetic acid (pKa = 2.902) and 0.555 moles of sodium bromoacetate to 1.00 L of solution.a) What is the pH of this solution?
- A buffer was made using 0.10 moles of A- and 0.01 moles of HA. If the pKa is 5.71, what is the pH of thebuffer?1.00g of acetylsalicylic acid is mixed with 120 mL of water. Then, 25.00 mL of the solution is transferred to 3 flasks each. Assuming the pH is 3.00, calculate the initial concentration of , the Ka and pKa.A buffer is made from 25.0mL of 1.0M CH3COOH and 25.0mL of 1.0M CH3COONa, what would be the pH of the buffer?