Write equations for the following separaions

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: A buffer solution is 0.100 M in both HC¬H5O2 and LICH5O2 and has a pH of 4.19. Which of the…

A: Buffer solution is the solution which resist change in pH on addition of small amount of acid and…

Q: buffer of pH = 7.5 is desired. Which two of the following compounds should be dissolved in water in…

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

Q: In general, which of the following will have the largest value? A. Equilbrium constant for the…

A: Ksp of an insoluble salt has largest equilibrium constant .

Q: The formation constant* of [M(CN) 6 ]4− is  2.50×1017 , where M is a generic metal. A  0.160  mole…

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Q: The acid ionization constant for Fe(H20)63+(aq) is 7.7x10-3. Calculate the pH of a 0.4630 M solution…

A:

Q: snip

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

Q: Calculate the buffer capacity of a buffer solution prepared by mixing 0.215M sodium acetate and…

A: Given =  Concentration of sodium acetate  = 0.215M Conc of acetic acid =  0.125M pKa =  4.76

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: 5. If the pH of the saturated solution Mg (OH)2 is equal to 10.5, calculate the Ksp of this salt.

A:

Q: Calculate the solubility of Mn(OH)2 in grams per liter when buffered at pH (a) 11.8

A: Introduction :  We have to calculate Solubility in grams per liter . Given :  pH = 11.8  From this…

Q: 1- In the Group 2 precipitations, the Sulfide Ion (S) is generated in an Acidic environment. If the…

A: Successive removal of H+ions from H2S is repersented by the followind two…

Q: If a 50.00 mL sample of 0.127 M nitrous acid is titrated with 17.55 mL of 0.102 M NaOH, what is the…

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Q: Consider Al(OH)3(s) + 3H+(aq) ↔ Al 3+(aq) + 3 H2O(l) a. Calculate K for this reaction. b. Calculate…

A: Given data :  pH of acid = 4.0  a)To get the K value we will devide concentration of products to the…

Q: A standardized iodine solution is used to titrate hydrazine sulfate in a sodium bicarbonate-…

A: A question based on concentration terms that is to be accomplished.

Q: The formation constant* of [M(CN)2]¯ is 5.30 × 10'8, where M is a generic metal. A 0.150 mole…

A: Given, [M(CN)2]- M+ + 2CN- ---> [M(CN)2]- Formation constant, Kf = 5.30 x 1018 Kf = [M(CN)2]- /…

Q: Calculate the buffer capacity of a buffer solution prepared by mixing 0.215M sodium acetate and…

A: Van Slyke developed an equation for determining buffer capacity.  Buffer capacity is defined by the…

Q: gravimetric analysis

A: In gravimetric analysis we add a Precipitating reagent into the analyte to make ppt then filter dry…

Q: Calculate the K for this reaction: 2Fe*3 + Pd 22FE*2(ag) + Pd*2 (aq) (aq) (aq) + Pd+2

A: For a reaction at equilibrium- K = [Product][Reactant]

Q: Compare the molar solubility of Mg(OH)2 in pure water with that in a solution buffered at pH 9.00.

A: The dissociation of Mg(OH)2 is Mg(OH)2 s⇋Mg2+ aq+ 2OH- aq. For pure water: Ksp = (s)(2s)2 =…

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

A:

Q: A buffer solution is made that is 0.482 M in HS and 0.482 M in NaHS. If Ka for H2S is 1.00 x 10-7,…

A: Given: Concentration of weak acid H2S = 0.482 M Concentration of conjugate base salt of weak acid…

Q: Express the equilibrium constant for the following reaction 10 PCI si 10 PCI 3- 10 0

A:

Q: The concentration of a K3[Fe(CN)6] solution is 0.15 M. Calculate the concentration of a solution of…

A: Given that, the concentration of a K3[Fe(CN)6] solution is 0.15 M.  We have to calculate the…

Q: 47. What is the pH of the buffer that results when 4.2 g of NH; (MW = 17.03 g/mol) and 4.6 g of…

A: The pH can be calculated as follows

Q: Calculate the solubility (in grams per 1.00 × 102 mL of solution) of magnesium hydroxide in a…

A: The solubility Ksp of Mg(OH)2 = 1.8 x 10-11Ksp = [Mg] [OH-]The concentration of OH- does not change…

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

A:

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

A: pH of a buffer solution can be calculated using H-H equation.

Q: Write a complete balanced net ionic equation where

A: The chemical reaction,  Cr(NO3)3 (aq.)+ NaOH(aq.) -----> Cr(OH)4- (aq.) + NaNO3(aq.)  So,…

Q: In the presence of CN, Fe+ forms the complex ion Fe(CN),*. The equilibrium concentrations of Fe+ and…

A: Equilibrium constant for any given reaction: Given data: Equilibrium concentration of Fe3+=8.5 x…

Q: 50 mL of a wastewater sample needs 21 mL of 0.1 M hydrochloric acid, HCI (MW = 36.5) to reduce its…

A: Given,  Volume of wastewater in mL = 50 mL Molarity of HCl = 0.1 M Volume of HCl in mL = 21 mL…

Q: Which of the following will result to the formation of a deep red solution. FeCl, (aq) + NH.SCN(aq)…

A: According to Le chaterlier's principle, when there is any disturbances in the equilibrium then the…

Q: The formation constant* of [M(CN)6]4− is 2.50×10^17, where M is a generic metal. A 0.170…

A:

Q: Calculate the pH of a 1.00 L buffer solution composed of O.250 M nitrous acid (HNO2, Ka = 6.92 x…

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Q: What do the solubility rules tell you about changing the temp and the pH of Alkaline Earth metals…

A: Solubility rules provides an idea on the solubility of different salts in water. The important…

Q: Calculate the concentration of ions in the following saturated solutions: (a) [I] in AgI solution…

A:

Q: |The solubility of cadmium oxalate, CdC2 04, in 0.150 M ammonia is 6.1 × 10-8 mol/L. What is the…

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Q: 16.72 Calculate the molar concentration of OH in a 0.724 M solu- tion of hypobromite ion (BrO"; K, =…

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Q: b) The complex ion of [Cd(en)." is formed by reacting aqueous solutions of cadmium(II), (Cd(H,O).",…

A: (i) Chemical equation for the formation of complex ion [Co(en)3]2+ is: (ii) The expression for…

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 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: The pH of buffer solution that has Ka = 6.23 x 105 and 5a, = 3a, is: а. 4.43 b. 4.03 С. 4.38 d. 3.98…

A: pH = d.  3.98

Q: Using the value of the formation constant for the complex ion Co(NH3)62+, calculate the dissociation…

A: A formation constant is an equilibrium constant for the formation of complex. Value of the formation…

Q: A solution is prepared by adding 0.090 mole of K3[Fe(CN)6] to 0.60 L of 2.0 M NaCN. Assuming no…

A: The equilibrium constant can be written as the ratio of concentration of products to the…

Q: Calculate the pH of the buffer solution produced from the addition of 0.030 L of 0.150 M KOH to…

A: For a buffer pH = pKa + log C2/c1

Q: molar solubility

A:

Q: 5. A solid sample of Zn(OH)2 is added to 0.350 L of 0.500 M aqueous HBr. The solution that remains…

A: Given that:  Molarity of HBr = 0.500M Volume of HBr solution = 0.350L Molarity = moles÷ volume…

Precipitation Titration

Precipitation analysis is used to analyze drugs, and to measure the salt content in food and beverages. It is an important concept from the examination point of view many practical questions are asked on the topic. This topic is significant in the professional exams for both undergraduate and graduate courses, especially for