How many grams of solid sodium cyanide should be added to 1.50 L of 0.172 M hydrocyanic acid solution to prepare a buffer with a pH of 8.570? (K, for hydrocyanic acid = 4.00x1010) 1.24 g sodium cyanide

How many grams of solid sodium cyanide should be added to 1.50 L of 0.172 M hydrocyanic acid solution to prepare a buffer with a pH of 8.570? (K, for hydrocyanic acid = 4.00x1010) 1.24 g sodium cyanide

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.7QAP

See similar textbooks

Related questions

Q: 4. (a) A laboratory technician dissolved 6.797 g of compound W (a non-electrolyte) in 15.00 mL of…

A: Please find the attachment.

Q: A buffer is prepared by adding 2.50g of lithium fluoride to 125 mL of 0.648M hydrofluoric acid. You…

A: Buffer is a substance which resists or very small change in the pH value of the solution when the…

Q: A buffer with a pH of 4.06 contains 0.19 M of sodium benzoate and 0.26 M of benzoic acid. What is…

A: Given information: pH of buffer solution = 4.06 Concentration of sodium benzoate = 0.19 M…

Q: Chemistry 3) How many grams of solid potassium fluoride should be added to 1.50 L of a 8.35x10-2 M…

A: Since it is a multiple questions ,so I solved first question, please post second question…

Q: A buffer is prepared by adding 2.50g of lithium fluoride to 125 mL of 0.648M hydrofluoric acid. You…

A: Buffer Solution It is a mixture of weak acid or base with their corresponding conjugate acid or…

Q: How many grams of solid sodium cyanide should be added to 1.00 L of 0.116 M hydrocyanic acid…

A: Given-> Volume of HCN = 1.00 L Molarity of HCN = 0.116 M pH = 9.990 Ka(HCN) = 4.00 × 10-10

Q: How many grams of solid potassium cyanide should be added to 1.00 L of a 0.193 M hydrocyanic acid…

A: As we know that Pka value for HCN = 9.2 Molar mass of KCN = 65 g/mol

Q: How many grams of solid ammonium chloride should be added to 2.00 L of a 0.221 M ammonia solution to…

Q: At 25 degrees Celsius, what is the pH of a buffer that contains 0.100 M dimethylammonium chloride…

A: dimethyl amine has pKa = 3.27

Q: How many moles of NH4Cl must be added to 3.0 L of aqueous 0.10 M NH3 to form a buffer whose pH is…

A: Adding ammonium chloride, NH4Cl, to an ammonia solution will effectively create a buffer solution…

Q: How many grams of sodium hypochlorite, NACIO, need to be added to 227 mL of a 0.185 M solution of…

Q: How many grams of solid sodium acetate should be added to 2.00 L of a 0.103 M acetic acid solution…

A: This problem is based on Handersen-Hasselbalch equation. Using this equation the concentration of…

Q: How many grams of solid sodium hypochlorite should be added to 1.50 L of a 0.185 M hypochlorous acid…

A: The given problem can be solved by using Henderson-Hasselbalch equation as; pH = pKa + log conjugate…

Q: buffer is made using 100.0 mL of 0.100 M CH_{3}3CH_{2}2COOH (propanoic acid) and 100.0 mL of 0.100…

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

Q: How many grams of solid sodium fluoride should be added to 1.50 L of a 0.169 M hydrofluoric acid…

Q: 2) How many grams of NaOH should be mixed with 5.4 g of oxalic acid (H,C.O.) and completed to 100 ml…

Q: The beaker contains 0.1 M acetic acid solution with methyl orange as an indicator. Another beaker on…

A: A buffer is formed when a weak acid is mixed with its conjugate base or weak base with its conjugate…

Q: You are asked to prepare 2.0 L of a HCN/NaCN buffer that has a pH of 9.8 and an osmotic pressure of…

A: Osmotic pressure can be calculated as:

Q: Please solve and show equations used and steps for a, b, & c

A: Molar solubility of Pb3(PO4)2 is calculated.

Q: 3.28 g of sodium acetate (82 g/mol) added to 400 mL of acetic acid to produce a buffer solution that…

A: Given 3.28 g of sodium acetate added to 400 ml of acetic acid to make buffer of pH =5 and pKa of…

Q: Consider a buffer made by adding 42.3 g of (CH3)2NH2I to 250.0 mL of 1.42 M (CH:)2NH (Kb = 5.4 x 10…

A: (CH3)2NH is a weak base and (CH3)2NH2I is its salt with a strong acid HI. Thus, the mixture is a…

Q: A 1.0-L buffer solution initially contains 0.25 mol of NH3 and 0.25 mol of NH4Cl. In order to…

A: First, the pKa value is calculated.

Q: Consider a buffer made by adding 32.7 g of (CH₃)₂NH₂I to 250.0 mL of 1.42 M (CH₃)₂NH (Kb = 5.4 x…

A: Number of Mole- Ratio of given mass of substance to the molar mass of substance is called number of…

Q: What is the pH of a buffer that contains 0.15 M CH3COOH and 0.10 M NaCH3COO (K, = 1.8 x 10$)?

A: Given : Concentration of weak acid CH3COOH = 0.15 M And concentration of conjugate base salt of weak…

Q: Consider a buffer made by adding 46.9 g of (CH₃)₂NH₂I to 250.0 mL of 1.42 M (CH₃)₂NH (Kb = 5.4 x…

A: Buffer is the solution that resists the change in pH. This solution tries to main the minimum…

Q: How many grams of solid sodium nitrite should be added to 1.00 L of a 0.227 M nitrous acid solution…

Q: How many grams of solid ammonium chloride should be added to 1.00 L of a 0.107 M ammonia solution to…

A: Calculate the value of pKa by using Kb value of ammonia,

Q: How many grams of solid sodium fluoride should be added to 0.500 L of a 0.185 M hydrofluoric acid…

Q: How many grams of solid potassium hypochlorite should be added to 0.500 L of a 0.273 M hypochlorous…

Q: How does a common ion affect the solubility of a compound? More specifically, how is the solubility…

A: The balanced chemical equation is given below,

Q: How many grams of solid sodium fluoride should be added to 2.00 L of a 9.37x10 M hydrofluoric acid…

Q: Tris(hydroxymethyl)aminomethane is a common base used to prepare buffers in biochemistry. Its Kb is…

A: To calculate pH of a basic buffer , we would first calculate its pOH using Henderson-Hassalbalch…

Q: A 1.0 liter solution contains 0.745 M hydrogen fluoride (HF) and 0.786 M sodium fluoride (NaF).…

Q: A volume of 500.0 mL of 0.110 M NaOH is added to 525 mL of 0.250 M weak acid (K, = 2.53 × 10–5).…

Q: A buffer with a pH of 4.09 contains 0.25 M of sodium benzoate and 0.32 M of benzoic acid. What is…

A: Number of mols = Volume of solution in L × Concentration inM Number of mols of sodium benzoate =…

Q: A 250.0-mL buffer solution initially contains 0.025 mol of HCHO2 and 0.025 mol of NaCHO2 . In…

A: A 250.0-mL buffer solution initially contains 0.025 mol of HCHO2 and 0.025 mol of NaCHO2. In order…

Q: How many grams of solid ammonium bromide should be added to 2.00 L of a 0.132 M ammonia solution to…

A: Interpretation- To determine how many grams of solid ammonium bromide should be added to 2.00 L of…

Q: How many grams of solid ammonium bromide should be added to 1.50 L of a 6.42x102 M ammonia solution…

Q: How many grams of solid ammonium chloride should be added to 2.00 L of a 5.44x10 M ammonia solution…

A: A buffer is a solution that can accept protons (by conjugate base) and donate protons (by acid) at…

Q: A volume of 500.0 mL of 0.180 M NaOH is added to 545 mL of 0.250 M weak acid (K, = 6.39 x 105). What…

Q: How many grams of solid potassium acetate should be added to 1.50 L of a 0.151 M acetic acid…

Q: A chemistry graduate student is given 300. mL of a 1.60M pyridine (C H,N) solution. Pyridine is a…

A: I am providing you an image that has solution of his question please have a look and try to…

Q: A chemistry graduate student is given 450. ml of a 1.10M dimethylamine (CH:) NH) solution.…

Q: A chemistry graduate student is given 250. mL of a 1.40M trimethylamine ((CH,) N) solution.…

Q: How many grams of solid sodium fluoride should be added to 0.500 L of a 9.49x10-2 M hydrofluoric…

Q: How many grams of NH4CI would have to be added to 250.0 mL of a 0.420 M NH3 solution to prepare a…

A: The minimum concentration of NH4Cl that must be present in the solution to have a pH of 10 is;…

Q: How many grams of solid sodium cyanide should be added to 1.50 L of a 0.233 M hydrocyanic acid…

Concept explainers

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.

Question

Is this the correct answer

How many grams of solid sodium cyanide should be added to 1.50 L of 0.172 M hydrocyanic acid solution to prepare a buffer with a pH of 8.570? (K, for hydrocyanic acid =
- 4.00×10-10)
1.24
g sodium cyanide

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this buffer.
Which of the following would form a buffer if added to 250.0 mL of 0.150 M SnF2? (a) 0.100 mol of HCl (b) 0.060 mol of HCI (c) 0.040 mol of HCl (d) 0.040 mol of NaOH (e) 0.040 mol of HF
You want to make a buffer with a pH of 10.00 from NH4+/NH3. (a) What must the [ NH4+ ]/[ NH3 ]ratio be? (b) How many moles of NH4Cl must be added to 465 mL of an aqueous solution of 1.24 M NH3 to give this pH? (c) How many milliliters of 0.236 M NH3 must be added to 2.08 g of NH4Cl to give this pH? (d) What volume of 0.499 M NH3 must be added to 395 mL, of 0.109 M NH4Cl to give this pH?
Calculate the pH change when 10.0 mL of 0.100-M NaOH is added to 90.0 mL pure water, and compare the pH change with that when the same amount of NaOH solution is added to 90.0 mL of a buffer consisting of 1.00-M NH3 and 1.00-M NH4Cl. Assume that the volumes are additive. Kb of NH3 = 1.8 × 10-5.
Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.
Marble is almost pure CaCO3. Acid rain has a devastating effect on marble statuary left outdoors. Assume that the reaction which occurs is CoCO3(s)+ H+(aq)Ca2+(aq)+HCO3(aq) Neglecting all other competing equilibria and using Tables 15.1 and 13.2, calculate (a) K for the reaction. (b) the molar solubility of CaCO3 in pure water. (c) the molar solubility of CaCO3 in acid rainwater with a pH of 4.00.
Consider the titration of butyric acid (HBut) with sodium hydroxide. In an experiment, 50.00 mL of 0.350 M butyric acid is titrated with 0.225 M NaOH. Ka HBut=1.5105. (a) Write a balanced net ionic equation for the reaction that takes place during titration. (b) What are the species present at the equivalence point? (c) What volume of sodium hydroxide is required to reach the equivalence point? (d) What is the pH of the solution before any NaOH is added? (e) What is the pH of the solution halfway to the equivalence point? (f) What is the pH of the solution at the equivalence point?
A buffer is made up of 0.300 L each of 0.500 M KH2PO4 and 0.317 M K2HPO4. Assuming that volumes are additive, calculate (a) the pH of the buffer. (b) the pH of the buffer after the addition of 0.0500 mol of HCl to 0.600 L of buffer. (c) the pH of the buffer after the addition of 0.0500 mol of NaOH to 0.600 L of buffer.
A buffer is made up of 239 mL of 0.187 M potassium hydrogen tartrate (KHC4H4O6) and 137 mL of 0.288 M potassium tartrate (K2C4H4O6). Ka for is (H2C4H4O6)4.55105. Assuming volumes are additive, calculate (a) the pH of the buffer. (b) the pH of the buffer after adding 0.0250 mol of HCI to 0.376 L of the buffer. (c) the pH of the buffer after adding 0.0250 mol of KOH to 0.376 L of the buffer.
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
A buffer solution with it pH of 12.00 consists of Na3PO4 and Na2HPO4. The volume of solution is 200.0 mL. (a) Which component of the buffer is present in a larger amount? (b) If the concentration of Na3PO4 is 0.400 M, what mass of Na2HPO4 is present? (c) Which component of the buffer must be added to change the pH to 12.25? What mass of that component is required?
A buffer is prepared using the butyric acid/butyrate (HC4H7O2/C4H7O2)acid-base pair. The ratio of acid to base is 2.2 and Ka for butyric acid is1.54105. (a) What is the pH of this buffer? (b) Enough strong base is added to convert 15% of butyric acid to the butyrate ion. What is the pH of the resulting solution? (c) Strong acid is added to the buffer to increase its pH. What must the acid/base ratio be so that the pH increases by exactly one unit (e.g., from 2 to 3) from the answer in (a)?