Find the theoretical λmax to test the complex formed by salicylic acid and Fe3+ ions

Q: will H3N titrate with 1.0M Ba(OH)2?

A: For any titration to be possible, one components needs to be acid and the other needs to be the base…

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 buffer solution is made with 0.15 M HA (Ka = 1.0 x 10-6) and 0.15 M A-. What is the pH of the…

A:

Q: You want 100.0 mL of a Buffer at pH = 9.10 and you have available the following; • 100.0 mL 1.00 M…

A: Henderson Equation: pH = pKa + log[salt]/[acid] Number of moles = Molarity x Volume (L)

Q: Find the molar solubility of Ag2CO3 since the concentration of [H3O+] is 1.0x10-11 M. (Ksp =…

A: given: concentration of [H3O+] = 1.0x10-11 M Ksp = 8.1x10-12  molar solubility of Ag2CO3 = ?…

Q: 3. Calculate the molar solubility of Cr (OH)3 in a solution buffered at (a) a pH of 5.00 and (b) a…

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Q: Calculate the concentration of CuS in a solution in which [H3O+] is held constant at 2.0×10-4 M

A:

Q: The pKa for Bis-Tris buffer is 6.5. What is the concentration of Bis-Tris Base if the pH is 6.9 and…

A: Answer:- This question is answered by using the simple concept of calculation of concentration of…

Q: Q: Why does adding HNO3 to the solution containing [Ag(NH;)2 make AgCl precipitate? Where does the…

A:

Q: You wish to prepare 2L of 1M sodium phosphate buffer, pH 8.0. You have stocks of 1M monobasic sodium…

A: Given: Concentration of NaH2PO4 = 1 M Concentration of Na2HPO4 = 1 M Volume of buffer solution = 2.0…

Q: 36. A 0.100 M aqueous solution of H₂SeO3 is titrated with 1.000 M NaOH solution. At the point marked…

A: Answer: Given curve is the titration curve of weak acid (H2SeO3) and strong base (NaOH) where weak…

Q: For the aqueous [Hg(NH3)4]2+ complex Kf = 1.8 * 1019 at 25°C. Suppose equal volumes of 0.0082M…

A: The formation of [Hg(NH3)4]2+  is shown as- Hg(NO3)2 (aq)+ 4NH3 (aq)→[Hg(NH3)4]2+…

Q: A sodium hydrogen carbonate/sodium carbonate buffer system is to be prepared with a pH of 9.7.  The…

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Q: solubility

A: 1- Ksp value for insoluble salt is very low but soluble salt is more because Solubility depends on…

Q: The solubility of PbBr2 is measured and found to be 4.19 g/L. Use this information to calculate a…

A: Solubility product of the reaction is equal to the product of concentration of the cations and…

Q: 1. Calculate the [H+] and the pH of a buffer solution that is 0.10 M in CH3COOH (Ka = 1.8 x 10-5)…

A: The  concentration of H+ and the pH of a buffer solution are calculated in step two.

Q: .2+ In aqueous solution the Ni ion forms a complex with four cyanide anions. Write the formation…

A: First step of the Balanced chemical equation for the formation of the complex:           Ni (H2O)42+…

Q: An EDTA solution is standardized against 0.3982 g of 99.99% CaCO3 (100.09 g/mol) dissolved in HCl…

A: given data  mass of CaCO3 is 0.3982g the volume of EDTA Is 38.00Ml pH is 10.0

Q: In aqueous solution the Ag ion forms a complex with two cyanide anions. Write the formation constant…

A: In the context of aqueous solutions, certain metal ions can form complexes with ligands, which are…

Q: 3. 50.00 mL of a solution of HNO₂ (Ka = 3.98x104) is combined with 50.00 mL of a solution of NaNO₂…

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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