Calculate the pH of a buffer that is 0.130 M in NaHCO3 and 0.335 M in Na2CO3.

Q: 1. Calculate the pH of a buffer system containing 1.0 M CH3COOH and 1.0 М СНЗСООNa.

A: According to guidelines i can answer only 1st question

Q: Carbonic acid (H2CO3) is a weak diprotic acid with a first ionization constant, Ka1 = 4.2 x 10–7.…

A: H2CO3  → H+ + HCO3-  It is given that,Ka1 = 4.2x10-7   pKa = -log10 Ka[H2CO3] = [HCO3–] = 0.100 M…

Q: A buffer is created by adding 0.321 moles of bromoacetic acid (pKa = 2.902) and 0.555 moles of…

A: Given that : Moles of acid (bromoacetic acid) = 0.321 moles Moles of salt (sodium bromoacetate) =…

Q: Calculate the pH of a buffer solution that is 0.339 M in NH3 (ammonia) and 0.143 M in NH4CI. pH =

A: Here we are required to find the pH of the buffer solution.

Q: Calculate the pH of a buffer that is 0.250 M in NaHCO3 and 0.280 M in Na2CO3.

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Q: What is the pH of a buffer that is 0.140 M in formic acid (HCHO2) and 0.010 M in potassium formate…

A: Given: [Acid] = 0.140 M [Salt] = 0.010 M Ka = 1.8 * 10-4   We have to calculate pH of buffer…

Q: Sodium acetate, NaCH;COO (82.0343 g/mol) is commonly used as acidic buffer solution. Estimate the…

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Q: What is the pH of a buffer solution containing 1.25 M NH₃ and 0.75 M NH₄NO₃? Note that the base…

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Q: A buffer solution is 0.486 M in NaH2PO4 and 0.394 M in Na, HPO4. If Ka for H2PO4¯ is 6.2 × 10¬8,…

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Q: A. Calculate the pH of a buffer made from 0.28 M HNO2 and 0.23 M NO2.. The Ka for HNO2 is 4.6 x…

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Q: A buffer system is set up with [HA] = 2[A-]. If pKa = 5.5, what is the pH of the buffer? %3D O A.…

A: Acidic buffer :-  A mixture of weak acid and its salt with strong base is called acidic buffer.  The…

Q: Calculate the pH of a buffer solution that is 0.496 M in C5H5N (pyridine) and 0.492 M in C5H5NHBr.…

A: GivenConcentration of the base pyridine, [C5H5N] =0.510MConcentration of the conjugate acid…

Q: Calculate the weights of Mg(OH)2 that will dissolve in  a) 250 mL of water b) 250 mL of a buffer…

A: Step-1 Let the solubility of Mg(OH)2 in 250 mL of water be ‘s’ Ksp = [S][2S]2 Ksp = 4S3 5.6 x 10-12…

Q: Calculate the solubility of Mn(OH)2 in grams per liter when buffered at pH (a) 7.0 ?

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Q: A buffered solution contains 0.50M H3CCO,H (acetic acid), which has a K. = 1.8 × 10-5, and 0.75M…

A: Buffer is a solution which resists the change in pH of a solution by the addition of acid or base.…

Q: Calculate the amounts of solids Na2HPO4 and NaH2PO4 needed to prepare 0.40 M, 1.5L of phosphate…

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Q: Calculate the pH of a buffer system containing 1.0 M CH3COOH and 1.2 M CH3COONa.

A: Ka for acid = 1.8 x 10-5  [CH3COOH] = 1.0 M [CH3COONa] = 1.2 M  PH = ?

Q: What is the pH of a buffer containing .0721 M Na2SO4 (aq) and .117 M NaHSO4 (aq)?

A: pH  of acidic buffer, pH = pKa+log([conjugate base]/[acid]).  pH  of acidic buffer, pH =…

Q: determine the pH on the buffer of (NH4) 2SO4 and NH4OH

A: Buffer solutions are those, that can resist the pH change on the addition of some acidic or basic…

Q: A buffer solution is prepared by dissolving  1.300 g  of ammonium chloride (NH4Cl) into  100.00 mL…

A: Mass of ammonium chloride is 1.3 g. Molar mass of ammonium chloride is 53.491 g/mol.

Q: Determine the pH of the buffer solution produced by the reaction of 5mL 0.1 M KOH and 30 mL 0.1 M…

A: Given-> Volume of KOH = 5 ml Molarity of KOH = 0.1 M Volume of CH3COOH = 30 ml Molarity of…

Q: What is the pH of a buffered solution that contains 0.25 M NHz and 0.22 M NH,CI?

A: Given,

Q: A buffer solution is prepared by taking 0.400 moles of acetic acid (pKa = 4.76) and 0.250 moles of…

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

Q: Calculate the change in pH when 0.0017 mol of HNO3 is added to 0.100 L of a buffer solution that is…

A: Answer: In this question we have to calculate the pH of the buffer solution before and after the…

Q: In an experiment on evaluation of antacid containing magnesium carbonate, a tablet weighing 2.50 g…

A: Given, mass of tablet = 2.50 g            molarity of HCl = 1.00 M            volume of HCl = 5.00…

Q: Show that the pH at the halfway point is equivalent to titration of a weak acid with a strong base…

A: The reaction of a weak acid with strong base will be like HA + BOH -------> BA + H2O where HA =…

Q: Calculate the pH of a buffer that is 0.225M HC2H3O2 and 0.162M KC2H3O2 . The Ka is 1.8 x 10-5.

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Q: If NaOClO3 is dissolved in pure water will the pH increase, decrease or stay the same?

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Q: 3. Determine the pH of the buffer solution below: 0.25 M NH3 and 0.30 M NH4+ with pka = 4.76

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Q: Calculate the pH of a buffer prepared by dissolving 21.5 g of benzoic acid (FW = 122.0 g/mol, Ka =…

A: Given: Weight of benzoic acid = 21.5 g Molar mass of benzoic acid = 122 g/mol Ka of benzoic acid =…

Q: 2. There is a phosphate buffer with 0.1 M of NaH₂PO4 0.1 M of Na₂HPO4. Calculate pH of buffer…

A: A buffer solution is a combination of two solutions - a weak acid solution and the salt of its…

Q: If a buffer solution contains 1.6 M acetic acid and 2.3 M sodium acetate, what is the pH of the…

A: Given  ka (Ionisation constant)                 = 1.8 × 10-5 Concentration of CH3COOH         = 1.6…

Q: What is the pH of a buffer that is .1 Molar in H2CO3 and 1M in NaHCO3?

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Q: Calculate the pH of a buffer system containing 2.0 M CH3COOH and 2.0 M CH3COOK.The pKa of CH3COOH is…

A: Concentration of CH3COOH=2.0M  Concentration of CH3COOH=2.0M  pKa of CH3COOH=4.74

Q: Consider a buffer solution that contains 3.87 M KClO2 which has a Ka value of 0.011 and 5.69 M…

A: Answer: Buffer solution is the type of solution that resists the change in its pH on adding small…

Q: What is the pH of a buffer that is 0.15 M in lactic acid [CH3CH(OH)COOH, or HC3H5O3] and 0.10 M in…

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Q: Calculate the pH of a buffer solution that is 0.200 M in HC2H3O2 and 0.100 M in NaC2H3O2.

A: The relation between pH of buffer and salt can be calculated using the Henderson-Hasselbalch…

Q: 6. "How many grams of HCI would need to be added to 25.0 ml of a 0.20 M solution of NaCICH₂CO₂ in…

A: Given,  Molarity of NaClCH2COO = 0.20 M  Volume of NaClCH2COO in mL = 25.0 mL  pH of the buffer =…

Q: Calculate the pH of the buffer system made up of 0.17 M NH3/0.47 M NH,CI.

A: Given : buffer solution of 0.17 M NH3 and 0.47 M NH4Cl  To calcxulate :- pH of  given buffer.

Q: show calculations for how the pH of each of these solutions would be determined. a. Buffer solution…

A: The question is  based on the concept of PH calculations. we have been given a weak acid and its…

Q: Calculate the molar solubility of Ni(OH)2 when buffered at pH 14.0

A: The solubility product of salt is a constant at a given temperature irrespective of the source from…

Q: Calculate the pH of a buffer solution that contains 0.79 M NaH2PO4 and 0.13M Na2HPO4   Calculate the…

A: The equilibrium reaction can be represented as,

Q: Calculate the theoretical pH for the following solutions . A buffer prepared by 50.0 mL of 0.20 M…

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Q: Calculate the pH of a buffer solution containing 0.92 M NaF and 0.44 M HE. The pKa of HF is 3.14.

A: Given that : Concentration of NaF = 0.92M Concentration of HF = 0.44M pKa = 3.14 pH of the buffer…

Q: A buffer solution is made by dissolving 0.230 moles of sodium hypochlorite in 1.00 L of 0.220 M…

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Q: Calculate the pH of a buffer that is 0.225 M HC2H3O2 and 0.162 M KC2H3O2. The Ka for HC2H302 is 1.8…

A: Given: Concentration of HC2H3O2 = 0.225 M Concentration of KC2H3O2 = 0.162 M Ka for HC2H3O2 =…

Q: Calculate the pH of a buffer solution containing 0.56 M NaF and 0.87 M HF. The pKa of HF is 3.14.

A:

Q: What is the pH of a buffer solution containing 1.25 M NH₃ and 0.78 M NH₄NO₃?

A: Given : Concentration of weak base NH3 = 1.25 M And concentration of conjugate acid salt of weak…

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.