Calculate the volume of concentrated ammonia and the weight of ammonium chloride you would have to take to prepare 175mL of a buffer at pH 8.5 if the final concentration of salt is to be 0.400 M.

Q: illustrates a typical neutralization titration, one between an HCl solution of unknown concentration…

A: Solution: Here we have HCl with unknown concetration and a standard NaOH . therefore, HCl will be…

Q: What is the pH of a hydrocyanic acid/sodium cyanide buffer in which the concentration of the weak…

A: we have to calculate pH of the given buffer solution

Q: Calculate the pH of a buffer solution prepared by dissolving 0.25 mol benzoic acid (CH,COOH) and…

A:

Q: The K, of hydroxylamine, NH,OH, is 1.10 x 108. A buffer solution is prepared by mixing 100.0 mL of a…

A: A buffer solution is a mixture of a weak acid and its conjugate base or a weak base and its…

Q: What must be the minimum concentration of hypoiodous acid in 1.00L buffer solution of a pH=10.72…

A:

Q: What is the pH of a buffer solution that is 0.20 M propionic acid and 0.46 M sodium propionate?

A: Interpretation: The pH of a buffer solution that is 0.20 M propionic acid and 0.46 M sodium…

Q: You are going to analyze an aspirin tablet using a UV-visible spectrophotometer. You crush an…

A: Blank solution means it has absence of analyte substance.

Q: In the lab, you perform an experiment in which you add HCIO4 and a beaker containing NH3. What will…

A: Equivalence point is the  point in titration at which the amount of titrant added is just enough to…

Q: An aqueous solution contains 0.464 M hypochlorous acid.How many mL of 0.364 M sodium hydroxide would…

A: The reaction as follows,

Q: What is the general rule in preparing a buffer with a high buffering capacity?

A: In the preparation of buffer (acidic buffer), a weak acid, such as acetic acid, and its salts, such…

Q: Describe a buffer with a low capacity and the same buffer with a greater capacity .

A:

Q: Calculate the molar concentration (M) of NaOH if 25.00 mL of NaOH required 36.68 mL of a 0.9500M…

A: Hcl+NaOH---->NaCl+H2O Neutralization reaction  M1V1/n1=M2V2/n2

Q: An aqueous solution contains 0.348 M nitrous acid. How many mL of 0.236 M sodium hydroxide would…

A:

Q: In titrating 40.0 mL of 0.10 M of HCI solution with 0.15 M of KOH solution, what would be the pH of…

A: We have to calculate the pH of solution.

Q: what do I need to calculate the theoretical pH if my buffer solution has 0.50 M of a ethyl alcohol…

A: Theoretical pH of a buffer solution is calculated using the Henderson-Hasselbalch Equation written…

Q: Why does buffer capacity increase as the concentration of buffer increases?

A: The solutions which have a nearly constant value of pH or they resist any change in pH value are…

Q: 1_Determine the volume of concentrated ammonia and the weight of ammonium chloride needed to prepare…

A:

Q: If the acceptable buffer range of the solution is ±0.10 pH units, calculate how many moles of H3O+…

A: pH drop is 0.1       then       initial pH = 9.6837       pH drop max = pH = 9.6837-0.1 = 9.5837…

Q: Calculate the pH of a buffer solution prepared from 0.155 mol of phosphoric acid, 0.250 mole of…

A: Given : Moles of Phosphoric acid i.e H3PO4 = 0.155 mol  Moles of conjugate base of phosphoric acid…

Q: The pH of a solution was monitored over the course of a titration. Below is the graph from the…

A: According to Henderson-Hasselbalch equation, pH = pKa + log[Salt][Acid]   Equivalence point is the…

Q: A 1-L unbuffered solution needs the pH adjusted from 7 to 1. How many mL of 12 molar HCI solution…

A: To find: Amount of 12M HCl solution required to change the pH of 1-liter unbuffered solution from pH…

Q: Describe how to prepare 1.0 L of buffer solution of pH 5.0, that can tolerate the addition of 0.3…

A: A buffer is a solution that resists the change in pH upon addition of a small amount of an acid (HA)…

Q: How many moles of NH4Cl must be added to 2.0 L of 0.10 m NH3 to form a buffer solution with a pH of…

A: Formula used :-  . pOH = pKb + log[salt]/[base] . pH + pOH = 14

Q: . (a) Which is the stronger base—the basic form of the indicator cresol red or         the basic…

A: Indicators are substances whose solutions change color due to changes in pH. They are usually weak…

Q: How many moles of potassium hydroxide would have to be added to 225 mL of a 0.478 M acetic acid…

A: Here KOH was added in acetic acid. pKa of acetic acid is 4.75 Now, 225mL 0.478M CH3COOH =…

Q: An aqueous solution contains 0.345 M dimethylamine ((CH3)2NH). How many mL of 0.370 M hydroiodic…

A:

Q: A 4.50−g quantity of a diprotic acid was dissolved in water and made up to exactly 250 mL. Calculate…

A: Given,Diprotic acid = 4.50 g in 250 mLKOH = 12.0 ml of 1.00 M.

Q: What must be the minimum concentration of hydrocyanic acid in 1.00L buffer solution of a pH 9.8…

A: Answer: Buffer solution is a type of solution in which on adding small quantity of acid or base, it…

Q: in titrating 40.0 mL of 0.10 M of HCI solution with 0.15 M of KOH solution, what would be the pH of…

A: The balanced chemical reaction is  HCl + NaOH ------> NaCl + H2O Number mmoles of HCl = molarity…

Q: How many grams of dry NH,Cl need to be added to 1.60 L of a 0.100 mol L- solution of ammonia, NH3 ,…

A: We have a buffer solution of base NH3 and salt NH4Cl.      From henderson hasselbalch equation ,…

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

A:

Q: A buffer solution is desired to be prepared by mixing 100 mL of 0.6M ammonia solution and 150 mL of…

A: Given, Volume of ammonia = 100 mL Molarity of ammonia = 0.6 M Volume of ammonium chloride = 150 mL…

Q: A chemist needs to prepare a buffer solution with pH = 10.00 and has both Na2CO3 and NaHCO3 in pure…

A: Given pH of buffer solution = 10.00 Volume of buffer solution = 1.00 L Total mass of salts = 10.0 g…

Q: A 4.50-g quantity of a diprotic acid was dissolved in water and made up to exactly 225 mL. Calculate…

A: Given : Mass of acid = 4.50 g Volume of solution made = 225 mL = 0.225 L…

Q: An aqueous solution contains 0.413 M hydrocyanic acid. How many mL of 0.319 M potassium hydroxide…

A:

Q: Calculate the pH of a solution formed by adding 2.00 grams of solid potassium cyanide, KCN, to 180.0…

A: Given,  adding 2.00 grams of solid potassium cyanide, KCN, to 180.0 ml of 0.340 M hydrocyanic acid…

Q: An aqueous solution contains 0.329 M methylamine (CH3NH2). How many mL of 0.305 M perchloric acid…

A:

Q: A solution is prepared that is initially 0.17 M in trimethylamine ((CH,),N), a weak base, and 0.20 M…

A:

Q: Preparation of buffers 1. Prepare 250ml of the following buffer solutions. Concentration Buffer…

A: Interpretation: To prepare 0.5 M, 250 mL of acetate buffer with a desired pH of 5.0.

Q: An aqueous solution contains 0.484 M methylamine (CH3NH2). How many mL of 0.388 M perchloric acid…

A:

Q: An aqueous solution contains 0.345 M dimethylamine ((CH3)2NH). How many mL of 0.370 M hydroiodic…

A:

Q: Determine the concentration of CH3COOH in a 40 mL solution if it takes 25 mL of a 0.035 M NaOH…

A: Acetic acid is a weak monoprotic acid and NaOH is monoprotic base so they reacts with each other in…

Q: A solution is prepared by mixing 80 mL of 0.2 M KH2PO4 and 120 mL of 0.2 M K2HPO4 . What is its pH?

A: Moles of KH2PO4 ( acid), = 0.2 M × 0.08 L = 0.016 mol   Moles of K2HPO4 (base), = 0.2 M × 0.120 L =…

Q: If you have 500 mL of a 0.10 M solution of the acid, what mass of the corresponding sodium salt of…

A:

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: Define the term Buffer-Capacity?

A: The amount of acid or base required to raise the pH of a buffer by unity is known as its buffer…

Q: Would a 0.010 M buffer solution or a 0.10 M buffer solution have a greater buffering capacity for…

A: Buffering capacity refers to the amount of added base or added acid that can be neutralized by a…

Q: Give the components of a buffer system and explain the requirements for a solution to be considered…

A: The question is based on the concept of buffer solution. We have to explain the concept of buffer…

Q: a. Suppose a solution contains 0.50 M NaHPO4 and 0.80 M NazHPO4. What pH should be expected for this…

A: Recall Henderson Hasselbalch equation to calculate pH of the given buffer solution          pH=pKa +…