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- The grid has six lettered boxes, each of which contains an item that may be used to answer the questions that follow. Items may be used more than once and there may be more than one correct item in response to a question. Place the letter(s) of the correct selection(s) on the appropriate line. Could dissolve Zn(OH)2 _____________ Could be used to prepare a buffer from __________ Halfway to the equivalence point in the titration of a weak, monoprotic acid with strong base ________ SO2-related atmospheric phenomenon __________ Species formed by a Lewis acid-base reaction ________ General condition required for precipitation to occur ________ [conj. base] = [conj. acid] in a buffer ___________Using chemistry how do you find/choose the right spf1. A 0.0250 M Ca(X)₂ has a pH of 8.049. Ca(X)₂ is composed of a Ca²+ cation and an unknown anion X, which undergoes hydrolysis. A. Write the balanced dissociation reaction of Ca(X)2 into its ions. Write your answer on your solution sheet B. Write the balanced hydrolysis reaction of the unknown anion, X. Write your answer on your solution sheet C. Calculate the K₁, or K, of X. D. Given the following K, values of different weak acids, determine the identity of X. Weak acids Ka HIO 2.00 x 10-11 HCN 6.17 x 10-10 CH₂COOH 1.80 x 105 HNO2 4.00 x 104
- A 40.00 mL sample of 0.1000 M diprotic malonic acid is titrated with 0.072 M KOH. What volume KOH must be added to give a pH of 5.56? Ka1 = 1.42 × 10–3 and Ka2 = 2.01 × 10–6. Show all of your work on your scratch paper and upload it as a comment to this quiz assignment. Correct!A student was titrating a solution of hydrazine (H₂NNH₂) with a nitric acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. The Kb for H₂NNH₂ is 3.0 x 10-6. Based on your ICE table and the equilibrium expression for Kb, set up the expression for Kb in order to determine the unknown concentrations. Each reaction participant must be represented by one tile. Do not combine terms. [0] [0.200 + x] [0.175 + x] [0.200] [0.200 -x] [0.175 -x] 0 1.70 Kb 4.77 x 10-1⁰ = 12.3 [0.0200] [0.100] [0.0200 + x] [0.0200 -x] 10.8 [0.140] 2 [0.100 + x] 2.10 x 10-² A student was titrating a solution of hydrazine (H₂NNH₂) with a nitric acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the…In the titration of 25.00 mL of a water sample, it took 20.590 mL of 3.150x 10−3 M EDTA solution to reach the endpoint. The total hardness is due to one or a combination of Ca2+, Mg2+, and Fe2+ in your sample. It is convenient to express this hardness as though it was entirely due to Ca2+. Making this assumption, determine the number of moles of Ca2+ present in the bottled water sample titrated. (enter your answer with 3 significant figures)
- You are directed to prepare 100 mL of a 500 mEq/L KOH standard. The primary standard used has a concentration of 0.400 Eq/L. When titrating your KOH solution, you discover that 4.0 mL of the primary standard reacted exactly with 5.0 mL of the KOH solution. a. What is the actual Eq/L concentration of the KOH solution? b. How many mEq are required to adjust the volume and concentration of the remaining 85 mL of KOH solution to 100 mL of a 500 mEq/L KOH solution? c. How many mL of 12 Eq/L KOH stock must be added in order to adjust the concentration of the KOH standard to 500 mEq/L?A 100.0 mL100.0 mL sample of natural water was titrated with NaOH.NaOH. The titration required 10.75 mL10.75 mL of 0.1477 M NaOH0.1477 M NaOH solution to reach a light pink phenolphthalein end point. Calculate the number of millimoles of NaOHNaOH required for the titration.17. Lime water has a hydronium ion content of 3.98 x 10-13. Find its pH.
- What mass of NaCN must be added to 1 L of 0.010 M Mg(NO3)2 in order to produce the first trace of Mg(OH)2?For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K data in the ALEKS Data tab. sp compound BaCO3 NaBr KC1 Does solubility change with pH? yes no yes no yes no pH = 7 highest solubility pH = 6 X pH = 5G.137.
