A buffer solution is 0.363 M in CH,COOH and 0.372 M in CH3COOK. If K, for CH,COOH is 1.8×10, what is the pH of this buffer solution?

Q: A buffer solution is 0.409 M in H2SO3 and 0.311 M in KHSO3. If Kal for H2SO3 is 1.7 x 10-2, what is…

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Q: The pH of a solution made by mixing 50.0 mL of 0.13 molar B, a weak base, with 20.0 mL of 0.19 M HCl…

A: The pOH of a solution by mixing weak base and HCl is calculated as,

Q: A buffer solution is 0.316 M in CH;COOH and 0.275 M in CH3COON . If K, for CH;COOH is 1.8×10³ , what…

A: Concentration of CH3COOH=0.316M Concentration of CH3COONa=0.275M Ka of CH3COOH=1.8×10^-5 pH=?

Q: 2. A buffer solution of volume 0.500 L contains 1.68 g NH3 and 4.05 g (NH);SOu. a) What is the pH of…

A: “Since you have asked multiple questions, we will solve the first question [Q2] for you. If you want…

Q: If a buffer solution is 0.110 M in a weak base (K, = 1.9 × 10-³) and 0.480 M in its conjugate acid,…

A: Given that:  [Base] = 0.110M  [Salt] = 0.480M  Kb = 1.9×10-5 Pkb = -logKb = -log(1.9×10-5) = 4.72…

Q: A students mistakenly titrates 25.0 mL of a 0.20 M H2SO4 solution, with 62.0 mL of a 0.15 M NaOH…

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Q: A buffer solution is 0.453 M in KH2PO4 and 0.271 M in K2HPO4. If Ka for H2PO4- is 6.2x10^-8, what is…

A: Buffer solutions show resistance to change its pH upon addition of strong acids or bases, which is a…

Q: A buffer, consisting of H2PO4- and HPO42-, helps control the pH of physiological fluids. Many…

A: The mass of NaH2PO4 is 6.5 g. The mass of Na2HPO4 is 8.0g. The Volume of the solution is 355 mL. We…

Q: t is the pH of a 0. M solutI 350 M solution of NaOH is added? The K, of HA is 4.3 x 10-4.

A: We have to tell which option is correct from given choices of options by telling what is the pH of…

Q: A buffer solution is 0.478 M in H3PO4  and 0.362 M in NaH2PO4 . If Ka1 for H3PO4  is 7.5 x 10^-3 ,…

A: According to the Henderson Hasselbalch equation is given by, Ph = Pka + log ([salt] / [acid] ) The…

Q: Acid strength decreases in the series HI > HSO4 > HF > HCN. Which of these equal molar salt…

A: Solution: We know as pH increases basic nature of compound increases. The pH of any salt depends on…

Q: When 42.6 mL of 0.100 M Ba(OH)2 is mixed with 98.6 mL of 0.200 M HCI, the reaction goes to…

A: A numerical problem based on pH concept, which is to be accomplished.

Q: A buffer solution is 0.438 M in HNO2 and 0.236 M in KNO2. If Ka for HNO2 is 4.5x10-4, what is the pH…

A: Given: concentration of HNO2 = 0.438 M  concentration of KNO2 = 0.236 M  Ka for HNO2 = 4.5 × 10-4…

Q: 1. A buffer solution is 0.200 M in HC,H;O2, a monoprotic acid, and 0.200 M in NaCH,O2. K, for the…

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Q: A 2.00 L solution contains 0.411 M NH3 and 0.660 M NHA. (The Kb of NH3 is 1.86 10-). What is the pH…

A: Given: Concentration of NH3 = 0.411 M Concentration of NH4A = 0.660 M And volume of solution = 2.00…

Q: If a buffer solution is 0.170 M in a weak base (?b=3.7×10−5) and 0.540 M in its conjugate acid, what…

A: In question it is not mentioned whether the base is monoprotic or polyprotic. Hence assuming it to…

Q: 5. Calculate the pH of a buffer system containing 1.0 M CH,COOH and 1.0 M CH,COON..

A: 5. Given information,      1.0 M CH3COOH and 1.0 M CH3COONa

Q: A buffer solution is 0.480 M in HCN and 0.361 M in NaCN . If K, for HCN is 4.0x10 what is the pH of…

A: This problem can be solved by using the buffer equation :…

Q: If a buffer solution is 0.560 M in a weak acid (Ka=5.3×10−6) and 0.120 M in its conjugate base, what…

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Q: If a buffer solution is 0.290 M in a weak base (K, = 1.4 × 10-5) and 0.580 M in its conjugate acid,…

A: pH of the buffer solution is determined by the Henderson-Hasselbalch equation as shown below: pH =…

Q: An aqueous solution of 0.057 M weak acid, HX, has a pH of 4.65. What is the pH of the solution if…

A: A buffer solution is made with a weak acid and its conjugate base, such solution resist the change…

Q: If a buffer solution is 0.290M in a weak acid (K = 7.2 x 10) and 0.600 M in its conjugate base, what…

A: By using this formula we can calculate the pH of solution .

Q: If the Kp of a weak base is 1.0 x 106, what is the pH of a 0.11 M solution of this base? pH =

A: Let us consider a base B, hydrolysis of the base is given below B + H2O ---> BH+ + OH- Now, at…

Q: what is the pH?

A: Given :-  Concentration of weak base = 0.120 M  Concentration of conjugate acid = 0.590 M  Kb = 5.9…

Q: A buffer solution contains 0.345 M KH,PO4 and 0.491 M Na HPO4. If 0.0261 moles of hydrobromic acid…

A: KH2PO4 and Na2HPO4 forms a buffer solution. When HBr is added to the solution, the net ionic…

Q: A buffer solution contains 0.436 M KH,PO4 and 0.317 M K,HPO4. If 0.0156 moles of sodium hydroxide…

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Q: How many grams of dry NH4C1 need to be added to 2.50 L of a 0.800 M solution of ammonia, NH3 , to…

A: NH3 + NH4Cl forms a basic buffer. For a basic buffer:  pOH = pKb + log c2/c1 pH + pOH = 14

Q: A buffer solution is 0.308 M in H2 C204 and 0.252 M in NaHC204. If Kal for H2C2O4 is 5.9 x 10¬ª,…

A: The pH of a buffer solution prepared by mixing a weak acid with the salt of its conjugate base can…

Q: A 0.15M solution of a weak base has a pH of 9.08. What is Kp for this weak base?

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Q: 100.0 mL of a 0.200 M H3PO4(aq) solution is titrated with 325.0 mL of a 0.100 M NaOH(aq) solution.…

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Q: An aqueous solution contains 0.396 M ethylamine (C2H5NH2). How many mL of 0.268 M perchloric acid…

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Q: A buffer solution is 0.372 M in NaHC204 and 0.323 M in Na2C₂O4. If K₂ for HC204 is 6.4E-5, what is…

A: Given: Concentration of NaHC2O4 is 0.372 M Concentration of Na2HC2O4 is 0.372 M Ka is 6.4×10-5 To…

Q: A buffer solution is 0.328 M in H₂C2O4 and 0.275 M in NaHC204. If Ka for H₂C₂O4 is 5.9E-2, what is…

A: In this question, we need to determine pH of the solution. Here given the values of concentration of…

Q: A buffer solution is 0.342 M in CH;COOH and 0.359 M in CH3COOK . If K, for CH,COOH is 1.8×10-5 ,…

A: Given: [CH3COOH] = 0.342 M [CH3COOK] = 0.359 M Ka of CH3COOH = 1.8×10-5

Q: A buffer solution is 0.390 M in H2 CO3 and 0.348 M in КНСОЗ. If Kal for H2 CO3 is 4.2 x 10-, what is…

A: Concentration of H2CO3 = 0.390 MConcentration of KHCO3 = 0.348 MKa1 of H2CO3 = 4.2×10-7

Q: A buffer solution is 0.389 M in H3PO4 and 0.351 M in NaH PO4. If Kal for H3PO4 is 7.5 x 10°, what is…

A: The given data is as follows:  The concentration of H3PO4 = 0.389 M The concentration of NaH2PO4 =…

Q: When 35.0 mL of 0.300 M hydrobromic acid and 35.0 mL of 0.300 M ammonia are combined, the pH of the…

A: Given molarity of HCI = 0.300 M Volume 35.0 mL = 0.035 L So, Number of moles of HC| = Molarity of…

Q: If a buffer solution is 0.210 M0.210 M in a weak acid (?a=5.0×10−5)Ka=5.0×10−5) and 0.490 M0.490 M…

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Q: If a buffer solution is 0.270 M in a weak acid (Ka = 7.5 x 10) and 0.570 M in its conjugate base,…

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Q: A buffer solution contains 0.254 M NaHSO3 and 0.348 M Na2SO3. If 0.0285 moles of hydroiodic acid are…

A: Calculate the initial pH of the given buffer solution using Henderson-Hasselbalch equation,

Q: An aqueous solution contains 0.305 M methylamine (CH3NH2). How many mL of 0.365 M hydroiodic acid…

A: Interpretation-  To determine the volume ( mL) of 0.365 M hydroiodic acid would have to be added to…

Q: If a buffer solution is 0.270 M in a weak base (K, = 1.3 × 10-) and 0.450 M in its conjugate acid,…

A: We have 0.27 M weak base , and 0.45 M of conjugate acid . We have to calculate the pH of this buffer…

Q: a) Calculate the pH of a buffer solution made by combining 3.S09g of NaOAc •3H,0 (Sodium Acstehe

A: Given: Mass of NaOAc.3H2O = 3.509 g Volume of HOAc =8.8 mL Volume of water added= 55.6 mL

Q: O Calculate the pH of a buffer that is 0.012 M C6H$COOH ( Ka= 6.3x10³) and 0.033 M NaCgH5COO.

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Q: A weak acid, HOCI, is in solution with dissolved sodium hypochlorite, NaOCl. If HCl is added which…

A: (1) Buffer of HOCl and NaOCl is a good example of acidic buffer solution. When any small amount of…

Q: A buffer solution is 0.485 M in HNO2 and 0.372 M in KNO2. If Ka for HNO2 is 4.5×10-4, what is the pH…

A: This problem is based on acidic buffer.    Acidic buffer are those which contain weak acid and salt…

Q: What is the pH of a buffer solution that is 0.24M NH3 and 0.20M NH4Cl?

A: Given,Concentration of NH3 = 0.24 MConcentration of NH4Cl = 0.20 MAmmonia (NH3), is a weak base with…

Q: For the buffer system in Problem no. 1, what will be the pH when (a) 15.0 ml of 0.500 M HCl and (b)…

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Q: Lactic acid has a K. of 2.502 x 103. A solution contains 0.275 M lactic acid and 0.375 M sodium…

A: Buffer solution: The mixture of lactic acid and sodium lactate act as a buffer solution. The…

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.