Part A: Calibration Curve Preparation (5 points)Solution NumberAbsorbance[Cu2+] (M)10.2850.120.5580.230.8280.341.0190.451.4180.5(a) Show calculations for the concentrations of the solutions entered in the table above(10 points)=

Step 1:To prepare a calibration curve, you'll first need to understand the relationship between…

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Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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КНР (ад) + NаОН (ад)- - NAKHP (aq) + H20 (1) Trial V; (mL) V; (mL) 33.87 45.73 2 A student masses out 1.019 grams of KHP, which is dissolved in 25.00 mL of DI water. This KHP solution is titrated with NAOH, as shown in the equation above. Calculate the molarity of the NaOH solution. RE FS F6 F7 FB F10
a) What is the solubility of copper(II) iodate, Cu(IO;)2? Ksp. = 1.4 x 107 at 25 °C %3D b) Will the solubility of Cu(IO3)2 (s) increase, decrease or remain the same if some solid Cu(NO:)2 is added? (copper(II) nitrate is very soluble and completely dissolves) c) Aqueous copper(II) ions, Cu²* to the reaction: (a0), react with aqueous ammonia to form a complex according Cu2+, (a0+ 4NH3 (a) [Cu(NH3)4]* (aq) with a formation constant, Ke= 1.2 x 1013 How will the addition of aqueous NH3 effect the solubility of Cu(IO3)2 (s)? (increase, decrease or no effect)
A solution was prepared by dissolving 367 mg of K3Fe(CN)6 (329.2 g/mol) in sufficient water to give 750.0 mL. Calculate (a) the molar analytical concentration and Normality of K3Fe(CN)6. (b) the molar concentration of K+. (c) the molar concentration of Fe(CN)63-. (d) the weight/volume percentage of K3Fe(CN)6.
Question 27 of 40 Submit Construct the expression for Ksp for solid Ba3(P04)2 in aqueous solution. Вa:(РOq)2(s) — З Ва" (аq) + 2 РО," (aq) 1 Based on your knowledge of how the solid will dissociate in aqueous solution, use the tiles to form the expression. Ksp ORESET [Ba3(PO4)2] 2[Ba3(PO4)2 3[Ba3(PO4)2 [Ba3(PO4)2l° [Ba3(PO4)21° [Ba*] 3[Ba] [Ba*j [Ba²*] 3[Ba2*] [Ba*j* [PO,*] 2[PO,] [PO,*]? [PO,] 2[PO,] [PO4]? 3[PO,*] [PO,*]°
For the aqueous Hg(NH,), complex K, = 1.8 × 101º at 25 °C. K; =1 Suppose equal volumes of 0.0010M Hg(NO,), solution and 0.20M NH, solution are mixed. Calculate the equilibrium molarity of aqueous Hg“ ion. 2 Round your answer to 2 significant digits. M ?
3+ 35 For the aqueous [Co (NH₂) complex K₁ = 1.58 × 10 at 25 °C. 3+ Suppose equal volumes of 0.0012 M Co(NO3), solution and 0.94 M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Co³* ion. Round your answer to 2 significant digits. M ? 20 x10 X S 2
Calculate the solubility of lead iodate (Pb(IO3)2, Ksp = 3.68 x 10-13).... (a) ... in pure water (b)... in a 0.100 M (Pb(NO3)2 (aq) solution
n/takeAssignment/takeCovalentActivity.do?locator=assignment-take Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. CH3COOH(aq) + H₂O(1) ⇒ H3O+ (aq) + CH3COO-(aq) K = Submit Answer 000 ORD F4 [Review Topics] [References] Use the References to access important values if needed for this question. F5 Retry Entire Group 9 more group attempts remaining Cengage Learning Cengage Technical Support MacBook Air F6 AA F7 DII F8 DD F9 F10 Previous Next Save and F12
112. Solutions of sodium thiosulfate are used to dissolve unexposed AgBr (Kp and-white film. What mass of AgBr can dissolve in 1.00 L of 0.500 M Na,S,O;? Ag* reacts with S,O,- to form a complex ion: = 5.0 × 10-13) in the developing process for black- Ag*(aq) + 2S,O;²-(aq) = Ag(S,O;),-(aq) K = 2.9 X 1013
3 Bal, (aq)+ 2 Nag POq Caq) 7 BalPO42 + l6 Nal laq • Consider the reaction of 30.0mL of 0.270M Balz with 20.0 mL of 0.3ISM Naz PO4. Lwhat quantity in meles of Balz are preset in the solution? are produced /What quantitg in moles of precipitate E ali Bal were consumed based on the balanced chomical equation? 6) What auantity in males of Na3 Pla aro present in soluction? d) What quantity in moles of precipitate are paduced if all the Naz PO, were cansumed based on the balanced chemi.cal equation? e) which reactant is limisting f What mass (in g) of precipitate is firemed when the limiting reactant is considered?
What is the concentration of limiting reaction solution of BaCl2? 3BaCl2 (aq) + 2NaPO4 (aq) -> Ba(PO4) (s) + 6NaCl (aq) Mass of precipitate is trial 1: 0.279g Mass of precipitate is trial 2: 0.487g Please complete trial 1&2
1. Calcium in a sample solution is determined by atomic absorption spectroscopy (AAS). A stock solution of calcium is prepared by dissolving 1.834 g CaCl, 2H,0 in water and diluting to 1 litre. From this stock solution, the second stock solution is prepared by the dilution factor of 10. Three standard solutions of calcium are prepared from the second stock solution with the following dilution factor: 20 (first standard solution), 10 (second standard solution) and 5 (third standard solution). A blank solution is prepared as well. Absorbance signals of AAS are as follows: 1.5 (blank solution), 10.6 (first standard solution), 20.1 (second standard solution), 38.5 (third standard solution), 29.6 (sample solution). (Molar mass; Ca = 40.00 g mol-, CI = 35.45 g mol-, 0 = 16.00 g mol-', H = 1.00 g mol-1) a. Construct ONE (1) plot that could be used to represent the calibration curve. b. From the plot of Q1a, determine the amount of calcium in parts per million.

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Part A: Calibration Curve Preparation (5 points) Solution Number Absorbance [Cu2+] (M) 1 0.285 0.1 2 0.558 0.2 3 0.828 0.3 4 1.019 0.4 5 1.418 0.5 (a) Show calculations for the concentrations of the solutions entered in the table above (10 points) =