Each row of the table below describes an aqueous solution at 25 °C.The second column of the table shows the initial components of the solution.• Use the checkboxes in the third column to explain the type of the initial solution.The fourth column describes a change in the solution.• Use the fifth column to predict how the change in the solution will change its pH.solution initial componentsinitial type(check all that apply)changeeffect of change on pH(check one)acidicpH higherAH₂Obasicadd NalpH lowerneutralpH the sameacidicpH higherBH₂O, KOHbasicadd H BrpH lowerneutralpH the sameacidicpH higherCH₂Obasicadd NaOHpH lowerneutralpH the sameacidicpH higherH2O, КОНbasicadd K BrpH lowerneutralpH the same

Given, The effect of change on pH when add acid, base and neutral compound to initial solutions is:

Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. initial type solution initial components (check all that apply) change effect of change on pH (check one) acidic O pH higher A H₂O basic add NaI O pH lower neutral O pH the same acidic O pH higher B H₂O, KOH basic add H Br O pH lower neutral O pH the same acidic O pH higher с H₂O basic add NaOH O pH lower neutral O pH the same acidic O pH higher D H₂O, KOH basic add K Br O pH lower neutral O pH the same

Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. initial type solution initial components (check all that apply) change effect of change on pH (check one) acidic O pH higher A H₂O basic add NaI O pH lower neutral O pH the same acidic O pH higher B H₂O, KOH basic add H Br O pH lower neutral O pH the same acidic O pH higher с H₂O basic add NaOH O pH lower neutral O pH the same acidic O pH higher D H₂O, KOH basic add K Br O pH lower neutral O pH the same

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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Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. Use the fifth column to predict how the change in the solution will change its pH. initial type solution initial components (check all that apply) effect of change on pH (check one) change acidic pH higher H,0, HI A basic add KI pH lower neutral pH the same acidic pH higher B H,0 basic add HBr pH lower neutral pH the same acidic pH higher H,0 basic add NaBr O pH lower neutral pH the same acidic pH higher H,0, HI basic add KOH pH lower neutral pH the same
Table 3. Ionization constants for orthophosphoric and citric acids. Acid К, (М) К2 (М) K3 (M) K,/K2 K/K3 Phosphoric 7.5 × 10-³ 6.2 × 10-8 2.2 × 10-13 1.2 × 10$ 2.8 × 105 Citric 6.0 × 10-4 1.5 × 10-5 4.0 × 10-7 40 38 Phosphoric acid (pKa, ~ 2.16, pka, - 7.2, and pka, ~12.32) Vs. Arsenic Acid (pKa, 2.0, pka, "6.8, and pka, "11.3) a) acid). (Please provide at least 1 sentence for each reason, and one could also provide a structure or reaction diagram to Describe 3 reasons why nature selected phosphate esters over other esters (arsenic-based ester or citric support your reasoning). b.) Explain why the following statement is true OR false.
Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. initial type (check all that apply) effect of change on pH (check one) solution initial components change acidic pH higher H,0 add HNO3 basic O pH lower neutral pH the same acidic O pH higher H,0, H Br add Na OH basic pH lower neutral pH the same acidic pH higher H,0 add KNO3 C basic pH lower neutral pH the same acidic pH higher H,0, H Br add Na Br basic pH lower neutral O pH the same O O 0O O 0 0 O C O000 000
Suppose a student performed a similar standardization titration experiment. Below is the calculated concentration of NaOH from each of their titrations. Titration #1 Titration #2 Titration #3 The concentration of NaOH (M) 0.9554 0.9540 0.9551 Using the 3 concentrations, calculate the average concentration of the student's NaOH solution and calculate the ± error in parts per thousand (ppt). Show the complete calculation. Express your final answer in the form of average (with units) ± error in ppt.
Recognizing common acids and bases Some soluble compounds are listed in the table below. Complete the table by filling in the name or chemical formula of each compound, whichever is missing. (If there is more than one way to name the compound, choose the name used when the compound is dissolved in water.) Also classify the compound using the checkboxes. compound NaI 0 12 sulfuric acid HCH₂ CO₂ ammonia name type of compound (check all that apply) strong weak strong weak acid acid base base ionic molecular O O O O O O × 3/5 00 S
Some chemical compounds are listed in the first column of the table below. Each compound is soluble in water. Imagine that a few tenths of a mole of each compound is dissolved in a liter of water. The important chemical species that would be present in this solution are written in the second column of the table. Use the checkboxes to classify each compound. compound HCI W Ba (OH), HC,H,O, KCI Explanation patric(most common) 1 Other place . с important species present when dissolved in water E н,о, ст. н.о Ba, OH, H₂O но, с.н,о.. нс.н, о,, H,о K, CI, H₂O Check $ 4 R type of compound (check all that apply) ionic molecular strong weak strong weak acid acid base base Speciation is happening because the two groups split and live in other places 0 % 5 0 0 0 0 0 T 0 0 0 G Search or type URL 0 0 0 0 X Y 0 0 0 0 S & 0 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Access 0.5 U * 00 8 9
Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. initial type solution initial components (check all that apply) change effect of change on pH (check one) acidic pH higher H₂O A basic add KNO3 pH lower neutral pH the same acidic pH higher B H₂O, NaOH basic add HClO4 pH lower neutral pH the same acidic pH higher C H₂O basic add KOH pH lower neutral pH the same acidic pH higher H₂O, NaOH basic add NaC104 pH lower neutral pH the same
Each row of the table below describes an aqueous solution at about 25 °C. Complete the table. That is, fill in any missing entries in the second and third columns. Round your entries for to 2 significant digits, and your entries for pH to 2 decimal places. [1,0] solution pH 6.9 x 10 mol/L O mol/L B 9.35 -5 5.3 x 10 mol/L
Each row of the table below describes an aqueous solution at about 25°C . Complete the table. That is, fill in any missing entries in the second and third columns. Be sure each entry you write includes the correct number of significant digits. solution H3O+ pH A ×7.010−9mol/L B mol/L 6.09 C 0.052mol/L
Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. initial type (check all that apply) effect of change on pH (check one) solution initial components change O acidic pH higher A II,0 basic add KCl pH lower neutral pH the same acidic pH higher H,0, , NaOH add NaNO, 3 рH lower B basic neutral pH the same acidic pH higher H,0 basic add KOH pH lower neutral pH the same acidic pH higher H,0, NaOH add HNO, рH lower basic neutral pH the same
Which of the following cations will form a weakly acidic solution? sodium calcium magnesium lithium aluminum Butanol and ethanol form a homogeneous solution. What is the strongest intermolecular force present? dispersion force dipole-dipole force hydrogen bonding ion-dipole force none of these
Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. alo initial type (check all that apply) effect of change on pH (check one) solution initial components change O acidic pH higher н,о, Кон A basic add H Cl pH lower O neutral O pH the same O acidic O pH higher В Н,0, КОН O basic add K CI O pH lower neutral O pH the same O acidic O pH higher H,0 O basic add Na ClO, O pH lower O neutral O pH the same O acidic O pH higher H,0 O basic add Na OH O pH lower O neutral O pH the same Explanation Check © 2021 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility