What is the pH of a buffer made from 0.350 mol of HBrO (Ka = 2.5 × 10-9) and 0.120 mol of KBrO in 2.0L of solution?

Q: What is the pH of a buffer that is composed of 121 mL of 0.10 M CH3COOH and 81 mL of 0.10 M…

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Q: What is the pH of a 498.2mL buffer solution with 0.239M HF and 66.55 grams of potassium fluoride?…

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Q: blood is 0.0016 M, determine the bicarbonate ion concentration required to buffer the pH of blood at…

A: We will use buffer equation

Q: A lactic acid/sodium lactate (HC3H5O3/NAC3H5O3) buffer is prepared to 0.104 mol L-1 HC3H5O3 and…

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Q: A solution contains 0.329 M HA (K₂ = 5.65 · 10−4) and 0.551 M NaA. What is the pH of this solution?…

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Q: 10.5 mL of 0.10M HF (ka+6.3x10-4) is titrated with 5.7 mL of 0.10M NaOH. What is the pH of the…

A: Moles of HF = (10.5*0.1)/1000 = 0.00105  Moles of NaOH = (5.7*0.1)/1000 = 0.00057  NaOH and HF will…

Q: Consider the titration of a 40.0 mL of 0.153 M weak acid HA (Ka = 2.7 x 10⁻⁸) with 0.100 M LiOH.…

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Q: A buffer solution is 0.396 M in HF and 0.233 M in KF. If Ka for HF is 7.2x10-4, what is the pH of…

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Q: A cereal contains 11.0g of sucrose (C₁₂H₂₂O₁₁) per 60.0 grams of cereal.How many grams of cereal…

A: The molar mass of sucrose (C12H22O11) is 342.2965 g/mol. According to the question, 11 g of sucrose…

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: 30.0 mL of 0.200 M HCN is placed in an Erlenmeyer flask.  After titrating the solution with 15.0 mL…

A: The reaction taking place is,

Q: How many grams of sodium hydroxide are needed to be added to 534 mL of 0.450 M HA solution to…

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Q: Calculate the pH of a buffer solution made of 0.35 M H2CO3 and 0.20 M NaHCO3. Ka=4.3x 10^-7 for…

A: pH is defined as negative logarithmic of concentration of hydronium ion

Q: What is the pH of a buffer solution containing 1.0 M hypochlorous acid (HClO, KA = 3.0 × 10^-8) and…

A: We can use Henderson-Hasselbalch equation which for a buffer solution that consists of weak acid and…

Q: A buffer is prepared by mixing 16 mL 1M CH3COONa and 4 mL 1M CH3COOH pKa = 4.74. Determine the pH…

A: Buffer capacity of buffer is a measure of magnitude of it`s resistance to change in the pH value on…

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: An industrial chemist studying bleaching and sterilizing prepares several hypochlorite buffers.…

A: Given : a buffer solution with  1) concentration of weak acid i.e HClO = 0.200 M 2) concentration of…

Q: What is the pH of the buffered created by dissolving 60.0g HCN (MM= 27.0253 g/mol) and 60.0g KCN…

A: The PH can be calculated as follows

Q: What is the pH of a buffer made from 0.120 mol of WCNO S(Ka=3.5* 10^ -4 ) and 0.410 mol of NaCNO in…

A: Given that,   Moles of WCNO  acid in 2.0 L  = 0.120 mol Moles of NaCNO base in 2.0 L  = 0.410 mol Ka…

Q: Lactic acid, (CH3CH(OH)COOH) is a common biomolecule which can accumulate inmuscles during intense…

A: The objective of this question is to calculate the pH of a buffer solution prepared by mixing lactic…

Q: If a buffer solution is 0.290 M in a weak base (K, = 1.4 × 10-5) and 0.580 M in its conjugate acid,…

A: pH of the buffer solution is determined by the Henderson-Hasselbalch equation as shown below: pH =…

Q: A buffer solution is prepared by dissolving 1.00 g of sodium acetate (CH3COONa) into 100.00 mL of a…

A: Given: The concentration of acetic acid is 0.100M. The volume of acetic acid is 100 mL. The…

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: Determine the pH of an equimolar buffer of ammonia and its conjugate base ion. (NH3; Kb = 1.8 x…

A: Solutions which are resisits it pH by addition of strong acid or base are called buffer solutions…

Q: Calculate the pH of a buffer solution that is 0.41 M in HOCl and 0.50 M in NaOCl. [Ka(HOCl) = 3.24 x…

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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: 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: What is the pH of a buffer made from 0.180 mol of HCNO (Ka = 3.5 × 10⁻⁴) and 0.410 mol of NaCNO in…

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Q: Identify the organic functional group of the product, the reaction type, and predict the functional…

A: Dehydration reaction: A dehydration reaction involves the loss of water molecule from the reactant…

Q: Calculate the pH of a buffer solution made from 1.000 g of sodium chlorate NaClO3 and 0.9561 g of…

A: Write the expression for pH. pH = pKa + log[salt][acid] Here, pKa is the negative logarithm of acid…

Q: A buffer solution is 0.405 M in HF and 0.200 M in KF. If Ka for HF is 7.2×10-4, what is the pH of…

A: Here given, Concentration of HF = 0.405 M Concentration of KF = 0.2 M Ka for HF = 7.2 x 10-4 We…

Q: A buffer solution is made that is 0.414 M in HClO and 0.414 M in KCIO. If Ka for HCIO is 3.50 ×…

A: The objective of this question us to calculate the pH value of the given reaction.

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: 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: 8. b) Calculate the pH of a buffer that was prepared by mixing 45 mL of 0.01M aqueous hydrocyanic…

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Q: What is the pH of a buffer made by combining 45.0 mL of 0.150 M nitrous acid and 20.0 mL of 0.175 M…

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Q: Calculate the pH of a buffer solution that contains 0.25 M benzoic acid (C,H5CO2H) and 0.15M sodium…

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Q: 100.0 ml of a 0.3 M solution of an unknown monoprotic weak acid has a Ka=1x10-6.  What mass of NaOH…

A: Volume of weak monoprotic weak acid = 100ml Molarity of weak monoprotic weak acid = 0.3M Ka = 1 x…

Q: A 80.00 mL solution initially contains 0.300 M HCN and 0.200 M KCN. What is the new pH after 1.0 mL…

A: To find the new pH after adding 1.0 mL of 2.5 M HCl to the solution, we need to consider the effect…

Q: What is the pH of a buffer solution that consists of 0.65 M HBrO and 0.38 M KBrO? Ka(HBrO) = 2.3 ×…

A: [acid]=[HBrO]=0.65M [conjugate base]=[kBrO]=0.38M Ka=2.3x10-9 pH=?

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.