What is the pH of a buffer made from 0.190 mol of HCNO (Ka = 3.5 x 10 4) and 0.410 mol of NaCNO in 2.0 L of solution?

Q: What is the pH of a buffer made from 0.220 mol of HCNO (Ka = 3.5 × 10 4) and 0.410 mol of NaCNO in…

A: Henderson's Equation:- This equation gives the pH of a buffer solution.  The number of moles of salt…

Q: What is the pH of a buffer made from 0.190 mol of HCNO (Ka = 3.5 x 10-4) and 0.410 mol of NaCNO in…

A: Henderson–Hasselbalch equation, pH = pKa + log [salt]/[acid]

Q: What is the pH of a buffer prepared by combining .92 moles of a weak base B, with .59 moles of…

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Q: Consider a buffer made by adding 132.8 g of NaC₇H₅O₂ to 300.0 mL of 2.31 M HC₇H₅O₂ (Ka = 6.3 x 10⁻⁵)…

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Q: You have a 0.500 L buffer solution composed of 0.47  M formic acid (HCOOH, Ka = 1.77 x 10¯4) and…

A: The acid ionization constant for acid is 1.77×10 -4.

Q: What is the pH of a 1.0 L buffer made with 0.300 mol of HF (Ka = 6.8 x 104) and 0.200 mol of NaF to…

A: The question is based on the concept of buffer. we have to calculate pH of the buffer after adding…

Q: Calculate the pH of a solution that is 0.45 M CH3COOH and 0.75 M NaCH3COO. Sodium acetate/acetic…

A: Buffer is a solution which consists of a weak acid and it's conjugate base or weak base and it's…

Q: How many grams of dry NH4Cl need to be added to 2.40 L of a 0.800 M solution of ammonia to prepare a…

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Q: buffer

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Q: Calculate the pH of a buffer that was prepared by mixing 90 mL of a 0.01M aqueous hydrocyanic acid…

A: HCN is a weak acid. In presence of base it produces it's conjugate base and form buffer solution.…

Q: To mimic a blood buffer, a scientist prepared 1.00 L buffer containing 0.0025 mol carbonic  acid,…

A: Given Ka = 4.3*10-7 concentration of H2CO3 = 0.0025 Concentration of HCO3- = 0.025

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

A: A buffer is made of a weak base and salt of that base. When an acid is added to the buffer, the base…

Q: At 25oC, a 1-L buffer solution is prepared by mixing acetic acid and sodium acetate. A) If the…

A: Use Henderson Hesselbalch's equation to get the pH of buffer solution having weak acid and its salt…

Q: What is the pH of a buffer made from 0.090 mol of HCNO (Ka = 3.5 × 10⁻⁴) and 0.410 mol of NaCNO in…

A: Moles of HCNO=0.090molMoles of NaCNO=0.410molVolume of…

Q: A buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M NaHCOO. What is the pH of this…

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Q: What is the pH of a buffer made from 0.350 mol of HBRO (Ка 3 (Ka = 2.5 x 10°) and 0.080 mol of KBRO…

A: Given : Moles of HBrO = 0.350 mol. Moles of KBrO = 0.080 mol. Ka of HBrO = 2.5 X 10-9  And volume of…

Q: How many grams of hydrofluoric acid, HF, should you add to a 1.65 L of a 2.65 M sodium fluoride…

A: Given: pH = 3.45 pKa = 7.1 x 10-4 Volume, V (NaF) = 1.65 L Molarity, M (NaF) = 2.65 M The strong…

Q: What is the pH of a buffer made from 0.580 mol of CH;NH2 (Kb = 4.4 x 10-4) and 0.220 mol of CH3NH31?

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Q: What is the pH of a buffer

A: Buffer is a solution of weak acid and base. the pH of buffer can not changes with addition or acid…

Q: What is the pH of a buffer made from 0.350 mol of HBrO (Ka = 2.5 × 10⁻⁹) and 0.150 mol of KBrO in…

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Q: What is the pH of a buffer prepared by adding 0.607 molof the weak acid HA to 0.609 molmol of NaA in…

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Q: What is the pH of a buffer made from 0.140 mol of HCNO (Ka = 3.5 × 10⁻⁴) and 0.410 mol of NaCNO in…

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Q: What is the pH of a buffer made from 0.350 mol of HBrO (Ka = 2.5 x 10-9) and 0.090 mol of KBrO in…

A: pKa = -log Ka = -log (2.5 x 10-9) = 9 -log2.5 = 9-0.40 =8.60 Henderson equation: pH = pKa +…

Q: A buffer is made using 50.00 mL of 0.7000 M HA (a weak acid, Ka = 1.000 x 10-5) and 50.00 mL of…

A: GIVEN: Initial concentration of HA=0.7000 M  Initial volume of HA =50.00 mL Initial concentration of…

Q: Consider a buffer made by adding 132.8 g of NaC,H;O2 to 300.0 mL of 1.31 M HC,H;O2 (Ka = 6.3 x 105)…

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Q: What would be the composition and pH of an ideal buffer prepared from lactic acid (CH3CHOHCO2H),…

A: The composition and pH of an ideal buffer prepared from lactic acid (CH3CHOHCO2H), (where the…

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: At 25oC, a 1-L buffer solution is prepared by mixing acetic acid and sodium acetate. A) If the…

A: Given: pH = 5 Ka of acetic acid = 1.8×10-5   Calculation for pKa of the acetic acid: Calculation…

Q: 3. (6)What is the pH of a buffer that is 0.12M lactic acid (HC3H5O3) and 0.1OM sodium lactate? Ka=…

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Q: 6. A buffer solution contains 0.1OM benzoic acid (C,H5COOH, Ka = 6.3 x 10) and 0.10M potassium…

A: pH can be calculated by using henderson equation  pH = pka + log (salt/ acid) Pka = - log 6.3 x10-5…

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: An acetic acid buffer contains 0.6 M CH3COOH and 0.6 M CH3COONA. (CH3COOH has a K, 1.76 x 105.) What…

A: Given- Concentration of CH3COOH= 0.6M Concentration of CH3COONa= 0.6M Ka of CH3COOH=1.76 ×10 -5…

Q: What is the pH of a buffer made from 0.350 mol of HBrO (Ka = 2.5 × 10⁻⁹) and 0.160 mol of KBrO in…

A: For HBrO , pKa = -log Ka = -log ( 2.5 × 10⁻⁹ ) = 9 - log2.5 = 9 - 0.40 = 8.60 For buffer : pH = pKa…

Q: 1. What is the pH of a buffer that contains 0.15 M CH,COOH and 0.10 M NACH,COO (K, = 1.8 x 10 )?

A: 1) Given, Concentration of CH3COOH solution = 0.15 M [CH3COOH] = 0.15 M Concentration of NaCH3COO…

Q: What is the pH at the equivalence point when 75.0 mL of a 0.225 M  solution of acetic acid (CH3COOH)…

A: We are having  the titration of weak acid with the strong base that will produce the salt of weak…

Q: A student set up a titration apparatus that involved using 25.9 mL of 1.57 M acetic acid. The acetic…

A: Given : volume of acetic acid = 25.9 ml Molarity of acetic acid = 1.57 M Molarity of NaOH =0.154 M…

Q: What is the pH of a buffer made from 0.220 mol of HCNO (Ka = 3.5 × 104) and 0.410 mol of NaCNO in…

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Q: Calculate the pH of a buffer solution made from 0.30 M hydrofluoric acid and 0.70 M sodium fluoride…

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Q: You have 500.0 mL of a buffer solution containing 0.15 M acetic acid (CH3COOH) and 0.25 M sodium…

A: Given, Concentration of Acetic Acid = [CH3COOH] = 0.15 M Concentration Sodium acetate = [CH3COONa] =…

Q: 4) Calculate the pH of a buffer that is 0.012 M C&H5COOH ( Ka= 6.3x10 5) and 0.033 M NaCsHsCOO.

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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…

Q: calculate the pH of a asolution that is made when 0.10 L of 0.24 M benzoic acid (pKa=4.19) and 0.050…

A: Benzoic acid is a weak acid and sodium hydroxide is a strong base. The reaction between them results…

Q: What is the pH of a mixture that contains 0.20 M Ca(OH)2 and 0.20 M LiOH?

A: Strong bases completely ionize when dissolved in water. Both the base, Ca (OH)2 and LIOH are strong…

Q: What is the pH of a 1.0 L buffer made with 0.300 mol of HF (Ka = 6.8 x 104) and 0.200 mol of NaF to…

A: they form a buffer solution.

Q: What is the pH of a buffer made from 0.200 mol of HCNO (Ka = 3.5 × 10⁻⁴) and 0.410 mol of NaCNO in…

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Q: What is the pH of a buffer made from 0.220 mol of HCNO (Ka = 3.5 × 10⁻⁴) and 0.410 mol of NaCNO in…

A: Henderson's equation for the calculation of buffer solution consisting of a weak acid and salt of…

Q: What is the pH of a buffer that contains 0.20 M CH 3COOH and 0.15 M NaCH 3COO?

A: Whenever the concentrations of the acid as well as its conjugate base, or the base and its…

Q: The Ka of hyperchlorous acid, HClO is 3.50 X 10-8. How many grams of NaClO (molar mass = 74.5…

A: 1- First calculate the concentration of NaClO :  Using the Henderson equation,  pH = pKa +…

Q: What is the pH of a buffer composed of 0.45 M C5H10NH and 0.65 M [C5H10NH2]Cl?

A: Formula for calculating pOH of a solution consisting of a weak base and its salt with a strong acid:…

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.