Mercury thiocyanate - Hg(SCN)2 - is slightly soluble in water.  Its Ksp is 2.8 x 10-20.   a.  Write the equilibrium reaction for mercury thiocyanate's dissolution.   b.  Write the equilibrium expression for the above reaction.   c.  In the titration of 50.00 mL of 0.0457 M Hg2+ with 0.200 M SCN-, show or calculate the following:      i.  The titration reaction        ii.  The volume of SCN- needed to reach the equivalence point (Ve).        iii.  pHg at 0.4 Ve        iv.  pHg at Ve        v.  pHg at 1.4 Ve

Q: pką values of phosphoric acid are 2.2, 7.2 and 12.7. A phosphate buffer of pH = 7.4 can be prepared…

A: pH of the buffer solution is 7.4 pKa values of phosphoric acid are 2.2, 7.2, 12.7

Q: Which one of the following indicators is best suited for titrating 0.05 M pyridine (pKb = 8.82) with…

A:

Q: 3.) What is the pH at the equivalence point for the titration of 50.0 mL 0.20 M nitrous acid by 0.20…

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Q: Which indicator would be the best to use for a titration between 0.30 M (CH3)2NH with 0.30 M HI? You…

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Q: A 25.00 mL solution of 0.08530 M Nal is titrated with 0.05030 M AgNO3. Given the Ksp of Agl is…

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A: Titration can be defined as a quantitative chemical analysis which is used to determine the…

Q: Sulfate buffer? Your laboratory is out of materials to make phosphate buffer and you are…

A: A buffer solution is formed by the weak acid and its conjugate base or weak base and its conjugate…

Q: How many grams of sodium borate (NaH2BO3) needs to be added to 1 L of 0.5 M of boric acid (H3BO3) to…

A: Answer :- 24.1 g  The mass of sodium borate (NaH2BO3) needs to be added to 1 L of 0.5 M boric acid…

Q: The Fajans titration uses an adsorption indicator to detect the endpoint of a titration in which a…

A: 1. An anionic dye binds to the positive surface of the precipitate. In this particular reaction.

Q: If you mix 2.4 mL of 2.000 M Fe³+ with 2.4 mL of 0.000883 M SCN, what is the concentration of…

A: 1 mole Fe3+ reacts with 1 mole SCN- to give 1 mole FeSCN2+ The equation is as follows: Fe3+ +  SCN-…

Q: Consider the dissolution of slightly soluble salt, PbCl2 (Ksp = 1.70 x 10-5): PbCl2(s)      ⇌…

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Q: S. Fe +3 + Fe (SCN) +2 State where the equilibrium shifted when Fe (NO3)3 Based on this equati SCN47…

A:

Q: Consider the reaction, PbF₂(s) = Pb²+ (aq) + 2F¯(aq) A. What will happen to the solubility of the…

A:

Q: Describe the preparation of 100 mL 0.050 M and 100 mL 0.0050 M phosphate buffer (both having pH =…

A: Stock solution of phosphate buffer of pH 6.5. Molarity of stock solution = 0.50M  Ka= 6.32 ×10-8 We…

Q: 2+ Calculate the mass of Cu (At.wt. 63) that titrated iodometrically with I ,then the liberated I,…

A: Molarity = no. of moles/ vol (Lt)

Q: 10 ml of a 1 M acetic acid (pK, = 4.75) are titrated with 0.5 M NaOH. a. Calculate the pH value of…

A: a. When 0 mL of the base NaOH is added, pH depends only on the concentration of the acid.

Q: 5. You were given with o.o25 M acetic acid and o.o25 M NaOH. You were then instructed to prepare a…

A: Given: Concentration of acetate ion in buffer = 0.02 M pH of buffer = 5.5  And the volume of buffer…

Q: Cag(PO4)2 (s)=3Ca2* (aq) + 2PO43- (aq) If, at equilibrium, a beaker contains 1.00 L of solution with…

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Q: How many grams of solid potassium nitrite should be added to 1.00 L of a 0.262 M nitrous acid…

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

Q: Calculate whether a precipitate will form if 1.75 mL of 0.70 M NH3 is added to 2L of 0.85 x 10-3 M…

A: The balanced chemical equation for the formation of zinc (II) hydroxide from ammonia and zinc…

Q: A 50.0-mL sample of 0.00200 M AgNO3 is added to 50.0 mL of 0.0100 M NaIO3. What is the equilibrium…

A:

Q: Calculate the change of pH of a buffer system with a pH of 7.323 if 0.217 mol potassium hydroxide…

A: If 0.217 mole of NaOH was added to the system  pH = 7.323Volume of phosphoric acid  525 mL = 0.525 L…

Q: 7. The formation constants for lead(II) oxalate are logKn=4.2; logKn=2.11. The Acid dissociation…

A:

Q: 8. Calculate the volume of 1.0M acetic acid and 1.0M sodium acetate solution needed to make 250 mL…

A: Given that, Molarity (concentration) of acetic acid = 1.0 M Molarity of sodium acetate = 1.0 M…

Q: Devon’s laboratory is out of material to make phosphate buffer. He is considering using sulfate to…

A: When a small amounts of acid or base is added to the solution, the buffer solution shows resistance…

Q: Answer the following questions regarding a 50.0 mL solution of 0.100 M solution of a weak acid, HY,…

A: 50.0 mL solution of 0.100 M solution of a weak acid, HY, Ka = 1.80 x 10-8 . The solution is titrated…

Q: . What is the pH of the solution obtained when 25.0 mL of 0.065M benzylamine, C7H7NH2, is titrated…

A: Given Concentration of benzyl amine = 0.065 M Volume of benzyl amine = 25.0 mL Concentration of HCl…

Q: What concentration of SO3 is in equilibrium with Ag₂ SO, (s) and 7.10 x 10-3 M Ag+? The Ksp of Ag₂…

A: Molarity of Ag+ = 7.10 × 10-3 M-> Ksp not given in question so used here from textbook.Ksp of…

Q: Calculate the pI after 50 mL. of 0.1 M Nal is titrated with 10.0 ml. 0.2 M AGNO3 solution? Given…

A:

Q: 2. Calculate the pH of buffer made of 0.500M NH3 and 0.456M NH4CI, pKb NH3 = 4.74. 3. Calculate the…

A: The Henderson hasselbalch equation is used to determine the pH of buffers. For acidic buffer, the…

Q: If the Ksp of BaF2 = 1.8 × 10-7 at 25 0C, calculate the molar solubility of BaF2 at 25 0C in: i.…

A:

Q: construct a theoretical curves for the titration of 25 ml of 0.1 n nh4Oh Hcl (pkb=4.74)  a. Write…

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

Q: Consider the following reaction: Ksp of CaCO3 = 4.9 × 10-9 Ka of HCO3¯= 4.7 × 10-11 CaCO3 (s) +…

A: K for the reaction is; CaCO3s↔Ca2+aq+CO32-aq, Ksp=Ca2+CO32- ...... iCO32-aq+H+aq↔HCO3-aq,…

Q: 5 You are given dropper bottles of the reagents listed below. Describe two ways to prepare a buffer…

A: Answer: Following solutions can be mixed: Formic acid + KOH Sodium formate and HCl

Q: Above what Fe2+ concentration will Fe(OH), precipitate from a buffer solution that has a pH of 9.65?…

A: Solubility Product Constant Ksp = Equilibrium Constant for a solution of solid to show the extent of…

Q: 3. A 100.0 mL sample of 0.10 M NH3 is titrated with 0.20 M HNO3. Determine the pH of the solution…

A: in this reaction NH3 and nitric acid both are limiting reagent because they are in same quantity so…

Q: Describe the preparation of 100 mL 0.050 M and 100 mL 0.0050 M phosphate buffer (both having pH =…

A: Given: The concentration of the stock phosphate buffer solution (pH 6.5) = 0.50 M The concentration…

Q: In the titration of a strong acid with a strong base, the pH of mixture after equivalence point is…

A: The correct alternative is option C [OH-] = ( NbVb - NaVa )/( Va + Vb ) & pH = 14 - pOH

Q: Mercury thiocyanate - Hg(SCN)2 - is slightly soluble in water.  Its Ksp is 2.8 x 10-20. In the…

A: Upon dilution, the number of moles in the solution remains constant whether the change in the…

Q: How would you use an experimentally determined Ksp value to calculate that Ag2CrO4 should…

A:

Q: 9. Sketch a titration curve for the titration of 0.100M NH3 (weak base) with 0,100 M HCI. Label the…

A:

Q: Enter your answer in the provided box. Calculate the pH at the equivalence point in the titration of…

A: Molarity of HCl = 0.330 M Molarity of methylamine = 0.150 M Volume of methylamine = 55.0 ml Kb = 4.4…

Q: The Ksp of AgCl is 1.82 x10-10 and the Ksp of AgSCN is 1.1 x10-12. Calculate the molar solubility of…

A: Given that, Ksp of AgCl = 1.82×10-10 Ksp of AgCl = 1.1×10-12 AgCl ionises in water to give Ag+ and…

Q: Calculate the pH using Henderson-Hasselbalch equation of a 50mL buffer solution made from 0.20 M…

A: Henderson-Hasselbalch equation                       pH = pKa + log[conjugate base][Acid]…

Q: B.) This is the titration curve of a formic acid (a weak acid) and a strong base. Give the name of…

A: Titration is defined as the process of determining the quantity of a substance A by adding substance…

Applications of Molecular Spectroscopy

When light sources pass through the diffraction grating then light splits into different wavelengths. The light source produces two types of patterns that are shown as destructive and non-destructive. The light source is in the form of quanta that is quantitation.