Calculate the pH of a buffer solution prepared by dissolving 0,48 mole of sodium fluoride (NaF) and 1.0 mole of hydrofluoric acid (HF) in enough water to make 1.0 liter of solution. [K,(HF) = 6,8 x 10ʻj Your answer should have 2 sig figs

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: At 22 °C, an excess amount of a generic metal hydroxide, M(OH),, is mixed with pure water. The…

A: In order to find Ksp of the salt we first write down the given data: pH= 10.34. The given salt is…

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: A buffer solution contains 0.371 Mhydrocyanic acid and 0.449 M potassium cyanide. If 0.0218 moles of…

A: pH = pKa + log[salt]/[acid]

Q: A chemistry graduate student is given 125. mL of a 1.10 M chlorous acid (HCIO,) solution. Chlorous…

A:

Q: A solution is prepared that is initially 0.12M in hydrofluoric acid (HF) and 0.061 M in sodium…

A:

Q: 40.0 mL of 0.20 M benzoic acid and 60.0 mL of 0.10 M sodium benzoate are combined in a large flask…

A:

Q: Question 3 I'm not sure how to solve this question.

A: We assume 1L of solution  Adding 16g of HBr  Moles of HBr added = 16/80.91 = 0.197 moles

Q: If a buffer solution is 0.240 M in a weak base (Kp = 5.5 x 10-) and 0.510 M in its conjugate acid,…

A: Henderson Hasselbalch equation is given by, pOH = pKb+log[conjugate acid][weak base] pKb is the…

Q: You are asked to prepare a pH = 3.00 buffer solution startingfrom 1.25 L of a 1.00 M solution of…

A: (a) Given: Concentration of HF – 1.00 M pH of the buffer solution = 3.00 Volume of solution = 1.25 L…

Q: What is the pH of a buffer solution that is 0.40 M in formic acid (HCHO2) and 0.90 M in sodium…

A: Given: pKa of formic acid = 3.74 Concentration of formic acid = 0.40 M Concentration of sodium…

Q: A solution is prepared that is initially 0.34M in acetic acid (HCH,CO, and 0.33M in potassium…

A: Molarity of acetic acid = 0.34 MMass of potassium acetate =0.33 M

Q: A solution is prepared that is initially 0.27 M in benzoic acid (HC,H,CO,) and 0.11 M in sodium…

A: The magnitude of an ionization reaction's equilibrium constant can be used to calculate the relative…

Q: At 22 °C, an excess amount of a generic metal hydroxide, ,M(OH)2, is mixed with pure water. The…

A: At 22 °C, an excess amount of a generic metal hydroxide, M(OH)2, is mixed with pure water. The…

Q: An aqueous solution contains 0.447 M dimethylamine ((CH3)2NH). How many mL of 0.246 M…

A: we need to find the volume of 0.246 M perchloric acid added to form the buffer solution with pH…

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…

A:

Q: In the laboratory a student measures the percent ionization of a 0.532 M solution of benzoic acid,…

A: Given: Initial concentration of benzoic acid = 0.532 M percent ionization = 1.05 %

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: 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: Consider a buffer solution that is 0.47 M HCN and 0.47 M NaCN. (Ka(HCN) = 4.9 × 10−10) Calculate…

A: After addition of 0.20 mol of NaOH the [ HCN ] = ( 0.47 - 0.20 ) = 0.27 M And [ NaCN ] = ( 0.47 +…

Q: If a buffer solution is 0.140 M in a weak base (K, = 5.6 x 10-) and 0.400 M in its conjugate acid,…

A:

Q: Q2. 0.5 M acetic acid in volume of 50 mL is titrated with 0.2 M NAOH after 50 ml of 0.2 M NaOH is…

A:

Q: A student dissolves a sample of a weak acid, HA, in 20.0 ml of H;O. The student then takes 5.6 mL of…

A: Given, Volume of water = 20.0 mL Volume of sample = 5.0 mL pH of final solution = 4.5

Q: A chemistry graduate student is given 100. mL of a 1.40M chlorous acid (HC1O,) solution. Chlorous…

A:

Q: Ex: Haw many moles of NaOH can be added to 1 liter of a solution 0.1 M in NH3 and 0.1 M in NH,Cl…

A: Answer is explained below.

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 student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a 1.14 M…

A: Given: Concentration of NaOH = 1.14 M Volume of HA solution used = 25.0 mL = 0.025 L…

Q: Which of the following acid/base conjugate pairs could you use to make a buffer solution with a pH…

A: Here we have to make a buffer solutions using conjugate acid/base pairs. The required pH is 12.55.

Q: A solution is formed by adding 3.60 grams of solid barium cyanide, Ba(CN)₂, to 250.0 ml of 0.170M…

A: To calculate the pH of the solution , we would first Calculate total concentration of CN- from both…

Q: Calculate the pH of a buffer that is 0.012 M C,H,COOH ( Ka= 6.3x10) and 0.033 M NaC,H;COO.

A:

Q: A chemistry graduate student is given 100. mL of a 0.80M chlorous acid (HCIO,) solution. Chlorous…

A: In the given problem, we are required to prepare a buffer having a pH of 1.37 using weak acid HClO2…

Q: A research wishes to prepare a buffer with a pH of 4.74 from weak acid HA (Ka = 2.57 x 105) and the…

A:

Q: A buffer solution contains 0.405 M NAHSO3 and 0.332 M Na,SO3. If 0.0248 moles of potassium hydroxide…

A: Given data, Molarity of NaHSO3 =0.405M Molarity of Na2SO3 = 0.332M Volume of buffer = 150mL = 0.150L…

Q: Calculate the equilibrium molar concentrations of trichloroacetic acid in an aqueous solution that…

A: Concentration in terms of molarity is defined as the moles of solute present per litre of the…

Q: What is the pH of a 100ml solution formed by adding 0.1mole NaOH to a buffer solution that contains…

A: Added base will neutralize acid and increase amount of the conjugate base salt in solution. Using…

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: 2.4. Consider a buffer solution that is 0.24 M NH3 and 0.20 M NH CI If 0.005 mol of NaOH is added to…

A: We would first Calculate initial pH of buffer solution. Then we need to calculate oH after adding…

Q: What mass of NaOH would be added to a one liter 0.200 M solution of acetic acid (pKa = 4.76) to…

A: Given : Volume of solution = 1 L  Concentration of acetic acid = 0.200 M And pH of solution = 4.76…

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: The K, for NH3 is 1.8 x 10-° at 25°C. Calculate the pH of a buffer solution made by mixing 45.7 mL…

A: Given data:- A buffer solution made by mixing 65.1 mL of 0.142 M NH3 with 38.0 mL of 0.172 M NH4Cl…

Q: A student prepares an 750.0 mL buffer solution with a pH of 4.85 by adding sodium acetate to a…

A: The buffer containing acetic acid (a weak acid) and sodium acetate (salt of acetic acid with NaOH)…

Q: A 50.0-mL sample of 0.50 M HCl is titrated with 0.50 M NaOH. What is the pH of the solution after…

A: We have given that  Concentration of HCl = 0.50 M and Volume = 50 mL = 0.05 L Concentration of NaOH…

Q: At 22 °C, an excess amount of a generic metal hydroxide, M(OH),2, is mixed with pure water. The…

A:

Q: Consider a solution of Hydrofluoric acid at equilibrium as follows:HF (aq)+H2O (l) F ̄ (aq)+H3O+…

A: #(a):  OH-(aq), being a base, will react with an acid.  Among all the species present in the…

Q: How many moles of sodium acetate must be added to 2.0 L of 0.10 M acetic acid to give a solution…

A: Calculation of no. of mol of acetic acid: No. of mol=Molarity×Volume=0.10 mol/L×2.0 L=0.2 mol…

Q: 1) Titrate in 26 ml of 2.2 M NaOH into 1200 ml of .5M HCO2H, what will the pH? How many more ml of…

A: Given: Volume of NaOH=26 ml Molarity of NaOH=2.2 M Volume of HCOOH=1200 ml Molarity of HCOOH=0.5 M…

Q: How many moles of sodium hydroxide would have to be added to 225 mL of a 0.332 M hydrocyanic acid…

A:

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.