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

Q: Calculate the pH of the buffer system containing 1.0M CH3COOH and 0.50M CH3COONa after the addition…

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Q: Calculate the solubility of Mn(OH)2 in grams per literwhen buffered at pH (a) 7.0, (b) 9.5, (c)…

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Q: Calculate the molar solubility of Ni(OH)2 when buffered at pH 8.0.

A: Given:   The pH value of Ni(OH)2 is 8.0. The value of Ksp is not given. Thus, so it is taken from…

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: Compare Tris and PBS as buffers in terms of temperature, ionic strength, and solvent effects.

A: Tris buffer is used as running buffer in agarose gel electrophoresis. Phosphate buffer saline is…

Q: Determine the pH of a 0.150 mol/L solution of NaCIO2 (sodium chlorite). The K, of HCIO2 is 1.10 x…

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Q: Write the expression for the solubility product constant for Pb(OH)2.

A: Solubility product constant ( Ksp):

Q: Calculate the molar solubility of iron(II) hydroxide in an aqueous solution buffered at pH = 6.07.

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

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Q: A buffer solution with a pH of 3.86 is prepared with 0.50 M formic acid and M sodium formate. The K,…

A: The formula of pH of a buffer solution is: pH=pKa+log[Salt][Acid]

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

A: pH is used to determine the concentration of hydronium ion.

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: Calculate the molar solubility of Ag₂CrO₄.

A: Let molar solubility of Ag₂CrO4 is S

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 consists of 0.25 M KHCO3 and 0.21 M K2CO3. Given that the K values for H2CO3 are, Ka1 = 4.5…

A: Given, 0.25 M KHCO3 0.21 M K2CO3 Ka1 = 4.5 x 10-7 and Ka2 = 4.7 x 10-11

Q: Based on the relation, Explain why does the solubility of Group II hydroxides increase and the…

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Q: Explain The Solubility of Amphoteric Metal Hydroxides?

A: Amphoteric compounds are those compounds which have the characters of both acids and bases. When…

Q: The molar solubility of lead phosphate in a 0.291 M ammonium phosphate solution is |M.

A: The question is based on the concept of common Ion effect.   it states that solubility of weak…

Q: Calculate the solubility of Mn(OH)2 in grams per liter when buffered at pH=9.7.

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Q: fore PbSO4 begins to precipitate. Assume

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Q: Calculate the molar solubility of CdCO3 in a buffer solution containing 0.115 M Na2CO3 and 0.120 M…

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Q: The titration curve of a weak acid, HnA has 3 inflection points at pH = 3.5, 6.7 and 10.3. If 0.1 M…

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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: The pK, value for HCIO is 7.46. Would a buffer prepared from HCIO and NaClO with a pH of 5.66 be…

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Q: A buffer is prepared by mixing 0.15 M NazHPO4 and 0.10 M NaH, PO4. K, for H3PO4 = 7.5 103 %3D Ka for…

A: The PH of buffer can be calculated as

Q: A buffer is made from 25.0mL of 1.0M CH3COOH and 25.0mL of 1.0M CH3COONa, what would be the pH of…

A: Since moles = concentration X volume of solution in L  Hence the moles of CH3COOH taken = 1 X 25 /…

Q: Calculate the pH of a buffer solution that contains 0.76 M NaH2PO4 and 0.28M Na2HPO4.   Calculate…

A: The equilibrium reaction can be represented as,

Q: What is the solubility product expression for Pb3(PO4)2

A: Given compound is Pb3(PO4)2. We have to calculate solubility product expression.

Q: Calculate the molar solubility of manganese hydroxide in a solution buffered at pH = 11.50. Mn(OH)2…

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Q: The EBT indicator changes color depending on the changes in pH of the solution during titration O…

A: False  EBT stands for Eriochrome Balck- T which is an indicator used in the complexometric titration…

Q: A solution is prepared by dissolving 0.23 mol of nitrous acid and 0.27 mol of sodium nitrite in…

A: Buffer solution - A solution whose pH is not altered to any great extent by the addition of small…

Q: A buffer solution is 0.100 M in both HC7H5O2 and LIC7H5O2 and has a pH of 4.19. Which of the…

A: The buffer solution is that can resist the small change in PH  by the addition of acid or base.

Q: A chemist needs to prepare a buffer solution with pH of 5.62, using HA and NaA. What ratio…

A: Buffer solution: The buffer solution is an aqueous solution consisting of a mixture of a weak acid…

Q: The Ka expression for the H,PO,/HPO;- buffer is given by the equation Ionic strength (µ, M) 0.005…

A: The Ka for the H2PO4-/HPO42- buffer is given by the equation: What is the pH of a 3:4 mixture of ...

Q: Calculate the molar solubility of Ni(OH)2 when buffered at pH 12.0

A: To calculate the molar solubility of Ni(OH)2 when pH 12.0. The solubility product of Ni(OH)2 is…

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: 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 solubility of Mn(OH), in grams per liter when buffered at pH = 9.7.

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Q: solubility product constant for Ca3(PO4)2-

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Q: Calculate the molar solubility of Ni(OH)2 when buffered atpH (a) 8.0, (b) 10.0, (c) 12.0.

A: In a balanced chemical reaction, the product of the equilibrium concentration of the ions of the…

Q: . What cations may be present in a pale blue solution that turns deep blue and forms a white…

A: solution- Cu2+ ion solution has pale blue solution and the reaction. the reaction between copper…

Q: Write a general expression for the solubility constant of a compound with the general formula AmXn.

A: Solubility constant of a compound is equal to the product of the concentrations of ions raised to…

Q: Calculate the molar solubilty of the following from its solubility product:  CaC2O4∙H2O

A: Let molar solubility be “x” CaC2O4.H2Oaq⇌Ca2+aq + C2O42- aq+ H2Ol

Q: The titration of Na,Se with HCI has the following qualitative profile. pH E F V2 mL HCI (a) Identify…

A: Point A : Na2Se  Point B : Na2Se + NaHSe  Point C : NaHSe ( first equivalence point)

Q: What is the precipitate formed when a solution of K2S is mixed with FeCl3?

A: Aqueous solution of Iron(III)chloride react with aquous potassium sulfide  to form precipitate.

Q: What of the following is the expression for the solubility product of Ba3(AsO4)2?

A: Given-> Ba3(AsO4)2

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.