A chemist needs to prepare a buffer solution with pH of 5.62, using HA and NaA. What ratio [base]/[acid] should be used in making the buffer? For HA, Ka= 1.4 x 10^-6

Q: How many moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer…

A: Introduction:  We have to calculate number of moles of NaOH . Given : pH = 3.70  Ka= 6.8 × 10-4

Q: with

A: pH = pKa + log( salt / Acid )  pH = -log(Ka) + log ( [A-] / [HA] )  Where : pKa = -log(Ka) and salt…

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 is made that is 0.310 M HCN and 0.316 M in NaCN. If Ka for HCN is 4.00 × 10-¹0,…

A: Given,molarity of HCN = 0.316 Mmolarity of NaCN = 0.316 MKa of HCN = 4.00 x 10-10 moles of NaOH =…

Q: A 1.0-L buffer solution contains 0.300 mol acid, HA, and 0.300 mol base, NaA. The value of K, for…

A: Weak acid and its salt with strong base will make a buffer whose PH can  be calculated with the help…

Q: A buffer is prepared using Lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm^3 of the 0.500…

A: Weak acid when present in a solution does not dissociate in its ions completely.

Q: Calculate the pH of a buffer comprised of 0.10 M hypochlorous acid and 0.080 M sodium hypochlorite.…

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

Q: Calculate the pH of a buffer solution containing 0.716 mol HA weak acid and 0.607 mol A- in 239.9 mL…

A: Answer:- This question is answered by using the simple concept of calculation of pH of a buffer…

Q: How many moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer…

A: Recall the reaction that will occur here HF + NaOH→ NaF + H2OHere,we recall Henderson Hasselbalch…

Q: What is the pH of a buffer prepared by combining 0.36 moles of a weak acid, HA, with 0.69 moles of…

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Q: How many moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer…

A:

Q: What quantity in moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a…

A:

Q: What is the pH of the buffer that occurs when 7.00 Mol of H2SO4 and 4.0 Mol of NaOH are diluted with…

A: A buffer solution generally consists of a weak acid and its salt. Buffer solution resists the change…

Q: How many grams of NaOH must be added to 1.50 L of a 0.400 M solution of oxoacetic acid (HCOCO2H) to…

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Q: During a titration, 10.0 ml of 0.135 M NaOH is added to 25.0 ml of 0.123 M CH3COOH. What is the pH…

A: Titration :- A titration is a technique where a solution of known concentration is used to determine…

Q: What quantity in moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a…

A:

Q: Calculate the pH of a buffer solution made by mixing a 0.37 M formic acid (HCOOH) with 0.23 M sodium…

A: pH of buffer solution=3.54Explanation:So,pH of buffer solution=3.54

Q: A buffer solution is made that is 0.319 M in HCN and 0.319 M in NaCN. (1) If Ka for HCN is…

A:

Q: Lactate is an important component in some intravenous solutions. Given pKa = 3.86 for lactic acid,…

A: pH = pKa  +  log ( [ conjugate base ]/[weak acid] ) ---------(i) pKa = 3.86 ( given) HC3H5O3…

Q: A bottle with 0.5 L of ammonia (NH3) solution that is 13.2% by mass has a density = 0.9430 g/mL. How…

A: Given, Volume of ammonia solution =0.5L Density of ammonia solution = 0.9430g/mL Mass % of ammonia…

Q: A buffer solution is prepared by adding 40.0 g of sodium acetate CH;COON to 500 mL of a 0.200 M…

A: The no of moles of sodium acetate and acetic acid are as follows:

Q: Calculate the pH of a buffer solution containing 0.659 mol HA weak acid and 0.602 mol A- in 288.3 mL…

A: We have to calculate the pH of solution

Q: How many moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer…

A:

Q: The pH of a bicarbonate-carbonic acid buffer is 6.18. Calculate the ratio of the concentration of…

A: The ratio of [H2CO3] to that of [HCO3-] is determined by using Henderson-Hasselbalch equation.

Q: Formic acid, HFor, has a Ka value of 1.8 x 10^-4. You need to prepare a buffer having a pH of 3.25…

A:

Q: What is the pH of a buffer made by combining 45.0 mL of 0.34 M nitrous acid and 60.0 mL of 0.48 M…

A: pH can be determined by using the information regarding concentration of the acid and the base.  pH…

Q: What is the pH of a buffer prepared by mixing 20.0 g of acetic acid (HC₂H30₂) and 20.0 g of sodium…

A: To determine pH of buffer solution Henderson Equation can be used depending on the type of buffer…

Q: a buffer solution is prepared via the combination of 1.246 M NH3 and 0.767 M NH4Cl (Ka=

A: Ka = 5.4954 x 10-10  PH = ?

Q: Calculate the pH of a buffer solution prepared by dissolving 0.400 mol of cyanic acid (HCNO) and…

A: Given  Number of mole of HCNO Acid      = 0.400 mole  Number of mole of sodium cyanate   Salt  =…

Q: Suppose you need to prepare a buffer system with a pH = 5.30 in the laboratory. The available acids…

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Q: What is the pH change when 28.8 mL of 0.0540 M NaOH is added to 70.1 mL of a buffer solution…

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Q: Acetic acid dissociates in water. If Keq = 1.80 x 10-5and the equilibrium concentrations of acetic…

A: Ka and C is given ,  C = 1.80* 10-5 Concentration of H+ and CH3COO-  will be same.

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…

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Q: Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is…

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Q: Let’s build a buffer using hypobromous acid (HBrO, Ka = 2.3×10−9) and hypobromite ion (BrO−). If…

A: Given: The concentration of hypobromous acid [HBrO]=0.100 M Ka=2.3×10−9 pKa= -log (2.3×10−9)…

Q: Calculate the pH of a buffer solution prepared by mixing 25 mL of 0.5 M lactic acid and 75 mL of 1.0…

A: Buffer solution  buffer solution is a solution that only changes slightly when an acid or a base is…

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. 

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.