Calculate how much of each solution you need to take to prepare 1 L of buffer solution with a pH of 9.45 using 0.3 M Na2CO3 and 0.2 M HCl (Ka1=4.3×10-7, Ka2=4.69x10-11)

Q: How many moles of CH₃NH₃Cl  need to be added to 200.0 mL of a 0.500 M solution of CH₃NH₂ (Kb for…

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Q: An amount H2SO4 (diprotic acid) was dissolved in enough water to make a 25.00 mL solution. Titration…

A: We have to calculate the Molarity of acid .

Q: A student is titrating 150.0 ml of a 0.300 M solution of lactic acid (pKa of lactic acid is 3.85)…

A: at equivalence point, moles of acid = moles of base

Q: 4. A buffer solution is prepared by dissolving 2.00 g each of benzoic acid, C6H5COOH (122.1 g/mol),…

A: 2.00 g each of the benzoic acid and sodium benzoate solution is prepared in 750.0 mL of water .…

Q: Calculate the pH of a solution that is 0.200 M in NH3 and 0.300 M in NH4Cl. Calculate the pH change…

A: Using Henderson-Hasselbalch equation: pH = pKa + log BaseAcid And, pOH = pKb + log AcidBase

Q: Using the table of the weak base below, you have chosen Ammonia as your weak base in the buffer…

A: Here we can solve the given question by applying Henderson Hassel-Blach equation to buffer solution.

Q: Answer the following three questions based on the information given below. Consider a buffer made…

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Q: You add 100.0 mL of 0.50 M NaOH to 50.0 mL of 1.00 M NH4CI. What is the pH of the resulting…

A: Ammonia(NH3) is a weak base whose base dissociation constant is given as Kb=1.8×10-5 while ammonium…

Q: 15.0 mL of 0.450 M formic acid (HCOOH, Ka=1.8x10-4) is titrated with 0.250 M NaOH. Calculate the pH…

A: The given information is as follows: The value of Ka of the formic acid = 1.8x10-4 The concentration…

Q: Consider a buffer solution comprised of HF and F-. The Ka of HF is 6.3 x 10-4. If the pH of the…

A: Weak acid are those acid which does not dissociate completely in aqueous solution. Here HF is weak…

Q: To a buffer containing 0.150 mol NH3 and 0.250 mol NH.* 0.050 mol of HCl (aq) is added. Calculate…

A: In this question, we will determine the pH of the Basic Buffer Solution.  The pH of a buffer…

Q: Human blood must have a pH between 7.35 and 7.45 - any deviation from this value causes serious…

A: Given range: 7.35-7.45 Fatal pH = 7.8

Q: What concentration of NaF do you need to add to a 0.15M HF solution to get a buffer solution pH of…

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Q: a) 50.00 mL of 0.1500 M NaOH is used to titrate 15.25 mL of H3PO4 to the endpoint (neutralization).…

A: The number of moles of a substance is defined as the mass of the substance upon its molar mass. The…

Q: What are the components of the buffer solution when 0.20 mol H3PO4 is made to react with 0.40 mol of…

A: Here 0.2mol of H3PO4 is made to react with 0.4 mol of NaOH . We have to find phosphate components…

Q: show the complete solution. - Calculate pH of a solution of a 0.10 M CH3COOH solution? Ka = 1.8 X…

A: Since you have posted a question with multiple sub questions and all are different . we will solve…

Q: A chemistry graduate student is given 125.mL of a 1.00M methylamine CH3NH2 solution. Methylamine is…

A: pH of buffer solutions can be calculated using Henderson-Hasselbalch equation. pOH of basic buffer…

Q: Calculate how much of each solution you need to take to prepare 1 L of buffer solution with a pH…

A: Buffer solutions are the solution which resist change in pH when small amount of acid or base is…

Q: Calculate the pH of the following solutions. (1)Tap water after boiling       (2)  0.0010 M NaOH…

A: Note - Since you have asked a question with multiple sub-parts, we will do the first three sub-parts…

Q: you mix together 50.0 mL of 0.25 M (NH4)2S and 50.0 mL of 0.20 M NH4Cl. What will the resulting…

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Q: A buffer solution consisting of 0.15 moles of ammonia dissolved in half a liter of water. How much…

A: The given solution is NH3/NH4Cl buffer. The pH of the basic buffer solution is to be determined…

Q: What are the components of the buffer solution when 0.20 mol H3PO4 is mixed with 0.30 mol of the…

A: Given statement is :  What are the components of the buffer solution when 0.20 mole H3PO4 is mixed…

Q: Determine the pH at the equivalence point when 65.0 mL of 1.22 M CH3ICOOH is mixed with 0.255 M KOH.…

A: We have to Determine the pH at the equivalence point when 65.0 mL of 1.22 M CH3ICOOH is mixed with…

Q: 0.5043 g of unknown acid was titrated with 27.35 mL of 0.5645 N NaOH solution. Calculate the…

A: Given-> Weight of unknown acid = 0.5043 gm Molecular weight = 98.00gm/mole Volume of NaOH = 27.35…

Q: Calculate the pH of a 0.250 M aqueous solution of CH3COOH. alculate the pH of a solution having…

A: Given,  i) The molarity of aqueous solution of   CH3COOH = 0.250 M.  The pH of the solution is: ii)…

Q: Determine the pH of each two-component solution.a. 0.0550 M in HI and 0.00850 M in HFb. 0.112 M in…

A:

Q: 1. Which of the following aqueous solutions are good buffer systems? .  0.35 M ammonia + 0.31 M…

A: Hi, we are supposed to answer one question. To get the remaining questions solved please mention…

Q: A buffer prepared by adding 115.0 mL of 0.17 M NH3 to 145.0 mL of 0.15 M NH4NO3. What is the pH of…

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Q: A student must make a buffer solution with a pH of 3.00. Determine which weak acid is the best…

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Q: 2 liters of water dissolve 2.24 liters of HCl measured under normal conditions. What is the pH of…

A: Volume of HCl = 2.24 litres  Moles of HCl = 2.24 / 22.4 = 0.1 mole  Concentration of HCl = 0.1 / 2 =…

Q: A solution of 150.0 mL of 0.50 M NH3 is titrated with 0.10 M HCl. Calculate the pH at 30% titration…

A: Millimoles of base=0.50 x 150.0 =75 mmol At 30% titration point : Millimoles of base converted into…

Q: To a buffer containing 0.150 mol NH3 and 0.250 mol NH4 0.050 mol of HCl (aq) is added. Calculate the…

A: pH of the resulting buffer solution can be calculated using Henderson hasselbalch equation.

Q: The graph here shows the pH curve for the titration of 25.00 mL of a 0.100-M monoprotic acid…

A: Concentration of acid [HA] = 0.100 M Concentration of base = 0.1 M  On the basis of titration curve…

Q: What is the pH of a 0.127 M solution of (CH3)2NH when it is titrated with 0.274 M of HCI to the…

A: At half equivalence point pH of the solution equal to pKa of weak acid  or  pKb of weak base

Q: Your answer is partially correct. A laboratory technician wants to determine the aspirin content of…

A: Given, The Ka= 3.0×10-4 Concentration = 10-5M

Q: How much of each solution is needed to prepare 1 L of buffer solution with a pH value of 9.45 using…

A: The question deals with the concept of preparation of  a buffer. A buffer is a solution which resist…

Q: If you have a ka = 8.25x10^-8, what buffer system will you use? Acetic acid (HC2H302) - Acetate ion…

A: Given: Ka of acid = 8.25 × 10-8

Q: You wish to titrate 38.00 mL of a 0.1680 M KOH solution with 0.1120 M HNO3. Calculate the pH after…

A: The question is based on the concept of titrations.   we are titrating  a strong acid with a strong…

Q: Calculate how much of each solution you need to take to prepare 1 L of buffer solution with a pH of…

A: Sodium carbonate and HCl react with each other as: Na2CO3+2HCl→2NaCl+H2CO3 ----(1)

Q: Using an acetate buffer system (CH3COOH & CH3COOK) with Ka = 1.77 x 10¯5, calculate how much of each…

A:

Q: You wish to titrate 38.00 mL of a 0.1680 M KOH solution with 0.1120 M HNO3. Calculate the pH after…

A: The pOH is calculated by the formula, pOH=-logOH The pH is calculated by the formula,…

Q: Use the scenario to answer the following question. A group of students working in a chemistry lab is…

A:

Q: Ten milliliters of 0.20 M AgNo3 is added 10ml of 0.10M NaCl calculate the concetration of Cl-…

A: Molarity of AgNO3 = 0.20 M Molarity of NaCl    = 0.10 M Volume of NaCl     = 10 mL

Q: A weak acid, HA, solution is titrated with NaOH. Calculate the pH of a solution when 25.0 mL of 0.40…

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Q: Which of the following set of reagents can be used for a buffer system? Select one or more: 0.10 M…

A: A buffer solution consists of a weak acid / weak base along with its conjugate base / conjugate…

Q: .  a buffer solution is 0.421 m in hcn and 0.281 m in kcn, if Ka for Hcn is 4.0 * 10^-10. what is…

A: The question is based on the concept of buffer solution.   A buffer is a solution which resist any…

Q: = H+ + HPO;- Ka = 6.2 x 10-8 = H+ + SO?- Ka = 1.3 x 10-2 From the systems above, identify the…

A: The question is based on the concept of buffer solution.   A buffer is a solution which resist any…

Q: Consider a 1.0 L buffer containing 0.093 mol L-1 HF and 0.119 mol L-1 F-. What is the pH of the…

A:

Q: Benzoic acid, HC7H5O2, has a Ka value of 6.4 x 10-5. B. Find the pH of a solution made by mixing…

A:

Q: If 2.02 g of H2C2O4.2H20 requires 29.8 mL of NaOH(aq) in a titration to reach the end point,…

A: Mass of H2C2O4.2H2O = 2.02 g  Volume of NaOH = 29.8 ml

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.