how many grams of sodium acetate trihydrate must be added to 50.0 ml of 0.250 M acetic acid to produce a solution with a pH of 4.60? (Ka=1.8*10-5)

Q: What will be the pH

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Q: 1.What mass of sodium formate must be added to 500.0 mL of 1.00 M formic acid to produce a buffer…

A: Given: The pH of formic acid is 3.50 The molarity of formic acid is 1 M. The volume is 500 mL. We…

Q: what volume of 0.10 M sodium acetate must be added to 20.0 ml of 0.20 M acetic acid to produce a…

A: The Henderson Hasselbalch equation for acidic buffer is given as :

Q: a 500 ml solution containing 0.01 m of acetic acid (ch3cooh) has a ph value of 3.38. how many…

A: For a weak acid such as CH3COOH, the concentration of H+ is given as, H+=Ka×C1/2 When NaOH is added…

Q: 0.100

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: What is the resulting pH when 125 mL of a 0.1 mol/L CH3COOH solution is titrated with 75 mL of a 0.1…

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Q: 1. a. What is the pH of a solution prepared by adding 25.0 mL of 0.10 M acetic acid (Ka = 1.8 x…

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Q: 11. What is the pH of a solution prepared by mixing 150 ml of 0.1 M HCl with 300 ml of 0.1 M sodium…

A: Hey, since there are multiple questions posted, we will answer first question. If you want any…

Q: If an acetic acid (CH3COOH)/sodium acetate (CH3COONa) buffer solution is prepared from 100 mL of…

A: Given : concentration of acetic acid = 0.1 M = concentration of sodium acetate And volume of acetic…

Q: What is the pH of a solution made by adding 23.5 g of KC2H3O2 to 400 mL of 0.80 M HC2H3O2? (Ka for…

A: Molarity of KC2H3O2 is calculated as follows:

Q: You want to prepare a pH = 4.50 buffer using sodium acetate and glacial acetic acid. You have on…

A:

Q: How do you prepare a 0.5L of 0.3M acetate buffer solution with a pH of 3.6? You are given acetic…

A: Here we have to prepare 0.5 L of 0.3M acetate buffer of pH =3.6 . Given material are acetic acid…

Q: You are asked to go into the lab and prepare an acetic acid- sodium acetate buffer solution with a…

A:

Q: A chemist titrates 250.0 mL of a 0.8331 M butanoic acid (HC,H,CO,) solution with 0.5749 M NaOH…

A: Molarity dilution equation: Given data: Concentration of butanoic acid=0.8331M. Volume of butanoic…

Q: What is the hydronium-ion concentration in a solution resulting from mixing 133 mL of 0.100 M HCN…

A: Answer:- This question is answered by using the simple concept of calculation of hydronium ion using…

Q: A 0.0640 M  solution of an organic acid has an [H+] of 1.75×10-3 M . What is the Ka value of the…

A: Given that [H+] is equal to 1.75×10-3 M and the initial concentration of an organic acid is 0.0640…

Q: 20.00 mL of 0.100 M sodium hydroxide is added to 40.00 mL of a 0.100 M acetic acid solution. The Ka…

A: Given data: Volume of sodium hydroxide = 20.00 mL = 0.02 L, Concentration of sodium hydroxide =…

Q: What is the pH (to two decimal places) of a 50.0 mL 0.15 M NH3 aqueous solution (at 25 °C) after…

A: Given-> Volume of NH3 = 50.0 ml Molarity of NH3 = 0.15 M Volume of HCl = 15.0 ml Molarity of HCl…

Q: What will be the pH when 50.0 ml of 2.00M carbonic acid is mixed 20.0 ml of 3.00 M sodium…

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Q: A 100.0 ml sample of a solution contains 2.00 x 10-3 M acetic acid (Ka= 1.8 x 10-5) and 1.00 M HCl.…

A: Since the dissociation constant (Ka ) of acetic acid is very low Hence very small amount of acetic…

Q: What is the pH of a solution prepared by mixing 150 mL of 0.10 M HCl with 300 mL of 0.20 M sodium…

A: Given, 150mL of 0.1M HCl 300mL of 0.1 NaOAc

Q: If you wanted to make 1.30 L of a solution of 80.0 mM acetate buffer at a pH of 5.20. How many moles…

A: We can use Henderson's Hasselbalch equation to solve this problem. That is, pH = pka + log…

Q: What is the pH after adding 25 mL of 0.1 M KOH solution to 50 mL of 0.100 M solution of propanoic…

A: Addition of the strong base OH- leads to the neutralization reaction. The number of moles of…

Q: A solution is made by mixing 175 ml of 0.100 M formic acid ( ka = 1.7 x 10^-4 ) with 175 ml of 0.100…

A: Volume of formic acid = 175 mL  Molarity of formic acid = 0.100 M  Volume of sodium formate = 175 mL…

Q: A chemist titrates 60.0 mL of a 0.1125 M hypochlorous acid (HCIO) solution with 0.7761 M KOH…

A: HClO is a weak acid and KOH is strong base   Calculating moles of HClO Volume in L x M = Moles…

Q: The next 9 questions are related to the titration of 20.00 mL of a 0.0750 M acetic acid solution…

A: The equation for neutralisation reaction between acetic acid and KOH is:

Q: What is the pH value of a buffer prepared by adding 10 mL of 0.1 M acetic acid to 20 mL of 0.1 M…

A: Given: Volume of acetic acid=10mL Molarity of acetic acid=0.1M Volume of sodium acetate=20mL…

Q: What is the pH of a solution made by adding 23.5 g of KC2H302 to 400 mL of 0.80 M HC2H302? (Ka for…

A:

Q: What is the pH of a buffer solution that is 0.26 M  propionic acid and 0.54 M  sodium propionate?…

A: Use acidic buffer equation to get the pH Pka= -log[Ka] Buffer mixture is formed by weak acid or weak…

Q: A 0.150 M NaOH solution is being used to titrate 50.0 mL of a 0.150 M ascorbic acid solution. a.…

A: Given,  Molarity of NaOH = 0.150 M Molarity of ascorbic acid = 0.150 M Volume of ascorbic acid =…

Q: Describe how you would accurately prepare 100.0 mL of a buffer solution with pH 4.7 using 1.0 M…

A: GIVEN: Concentration of acetic acid = 1.0 M Concentration of NaOH = 1.0 M Volume of buffer solution…

Q: You are making a buffer solution in the lab by combining the weak acid H2PO4- with its conjugate…

A:

Q: What is the pH of a buffer solution prepared by dissolving 0.10 mol of sodium acetate (NaC2H3O2) and…

A: Ka = 1.8 × 10-5 pKa = - log Ka        = - log (1.8 × 10-5)        = 4.745.

Q: A solution that is made by mixing 50.0 mL of 0.15 M acetic acid and 50.0 mL of 0.20 M sodium…

A: Ka of the acetic acid is 1.8×10-5 M. pKa of the acetic acid can be calculated as follows:

Q: A chemist titrates 110.0 mL of a 0.3453 M methylamine (CH3NH₂) solution with 0.7011 M HCl solution…

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Q: Draw a titration of (25) ml of Hcl acid (0.1M) with (NaoH) solution (0.1M) when adding the following…

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Q: What is the pH of a solution created by mixing 25.00 mL of 0.10 M formic acid and 25.00 mL of 0.10 M…

A:

Q: What is the pH at 25°C of a solution that results from mixing equal volumes of a 0.0500 M solution…

A: The pH of a solution is related to the acid dissociation constant by the Henderson-Hasselbalch…

Q: Calculate the pH of a solution that is 0.279 M  acetic acid and 0.190 M  sodium acetate.The Ka of…

A:

Q: Calculate the mass of sodium acetate that must be added to 500.0 mL of 0.760 Macetic acid to form a…

A:

Q: 10.0 mL of 0.400 M NaOH is added to 20.0 mL of 0.50 M CH3COOH. Calculate the pH of the resulting…

A: Generally pH is potency of H plus ion concentration. The formula of pH is the negative of logarithm…

Q: 2. A solution prepared by dissolving 2.25 g HA (MW = 51.0) and 4.00 g of NaA in 500 ml of solution…

A: Buffer solution :-      A buffer solution is one which resists changes in pH when small quantities…

Q: What is the pH of a buffer that is 0.12 M in lactic acid [CH3CH(OH)COOH, or HC3H5O3] and 0.10 M in…

A: The acid ionization constant for lactic acid is 1.4×10 -4.

Q: How many ml of 0.2 M HCl needs to be added to 100.0 ml of 0.2 M Sodium acetate (kb for acetate is…

A: In this question, we want to determine the volume of HCl in mL unit. You can see details Solution…

Q: What is the pH at 25°C of a solution that results from mixing equal volumes of a 0.0500 M solution…

A: The Henderson–Hasselbalch equation shows the pH of a solution which have a mixture of the two…

Q: What mass of sodium formate must be added to 500.0 mL of 1.00 M formic acid to produce a buffer…

A:

Q: (1). What will be the pH when 50.0 ml of 2.00 M carbonic acid is mixed 20.0 ml of 3.00 M sodium…

A: #1:  Given the volume of 2.00 M carbonic acid, H2CO3 = 50.0 mL * (1L/1000 mL) = 0.050 L => moles…

Q: What is the value of Q when the solution contains 2.00 x 10¬³M Ca2+ and 3.00 x 10-² M SO4²-?

A: To find Q?

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.