Pure water is neutral in pH or has a pH value of exactly 7.00. How does the pH of pure water vary when it undergoes distillation and boiling? Show the important equations if necessary, to explain why distilled and boiled water deviate from the neutral pH.
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Pure water is neutral in pH or has a pH value of exactly 7.00. How does the pH of pure water vary when it undergoes distillation and boiling? Show the important equations if necessary, to explain why distilled and boiled water deviate from the neutral pH.
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- Row 1: Your answer is incorrect. • Row 2: Your answer is incorrect. Row 4: Your answer is incorrect. The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that NH, is a weak base. 1.3 mol of HI is added to 1.0 L of a 1.3MNH, solution. 0.22 mol of HNO, is added to 1.0 1. of a solution that is 1.1M in both NH, and NH Br. ✔ acids: NH, H,O bases: 11,0, NHL, other: I acids: NH H bases: NH, other: NO, Br a S da X 0.0.1. Pure water is neutral in pH or has a pH value of exactly 7.00. How does the pH of pure water vary when it undergoes distillation and boiling? Show the important equations if necessary, to explain why distilled and boiled water deviate from the neutral pH.A drop of bromthymol blue and a drop of phenolphthalein are added to a beaker of distilled water. What is the resulting color of the water?
- An important aspect in the practice of pharmacy is to control the pH in solution for solubility of the drug. True FalseWrite the dissolution equation showing how solid lithium carbonate breaks up into ions in water; it is a weak electrolyteSome 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. type of compound (check all that apply) compound important species present when dissolved in water ionic molecular strong weak strong weak acid acid base base NaClO4 Na, CIO, H₂O 0 0 0 ΗΝΟ, H₂O, NO₂, HNO₂, H₂O 0 0 0 0 0 NaOH Na, OH, H₂O 0 0 0 0 0 NH₁₂ NH, OH, NH3, H₂O 0 Give detailed Solution with explanation needed of each..don't give Handwritten answer
- 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. type of compound (check all that apply) compound Important species present when dissolved in water ionic molecular strong weak strong weak acid acid base base 2+ Ba(OH)₂ Ba, OH, H₂O 0 0 CHẠNH, C₂H₂NH₂, OH, C₂H₂NH₂, H₂O но 0 0 0 0 + ΚΙ K, I, H₂O NaOH Na, OH, H₂O 0 0 X □ 3 ?Consider the following chemical equilibrium for the weak base CN in water: CN- (aq) + H₂O(1) = HCN (aq) + OH(aq). Which of the following statements is correct when more water is evaporated from system? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a b C d pH will go up; [OH-] will go up; net amount of OH will go up pH will go down; [OH-]will go up; net amount of OH will go down pH will go down; [OH-]will go down; net amount of OH will go down pH will go up; [OH-] will go up; net amount of OH will go downEach 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 components initial type (check all that apply) change effect of change on pH (check one) O acidic A H₂O, KOH basic ○ pH higher add KI O pH lower neutral acidic B H₂O basic add H CIO4 O neutral ☐ acidic C H₂O ☐ basic add Na CIO O neutral acidic O pH the same O pH higher O pH lower O pH the same O pH higher O pH lower O pH the same O pH higher D H₂O, KOH basic add HI O pH lower Oneutral 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. solution initial components initial type (check all that apply) change effect of change on pH (check one) acidic pH higher H₂O add HClO4 basic pH lower neutral pH the same acidic pH higher B H₂O, HBr basic add KOH pH lower neutral pH the same acidic pH higher с H₂O, HBr basic add K Br pH lower neutral pH the same acidic pH higher D H₂O basic add NaC104 pH lower neutral pH the sameEach 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 components initial type (check all that apply) change effect of change on pH (check one) acidic pH higher A H₂O basic add Nal pH lower neutral pH the same acidic pH higher B H₂O, KOH basic add H Br pH lower neutral pH the same acidic pH higher C H₂O basic add NaOH pH lower neutral pH the same acidic pH higher H2O, КОН basic add K Br pH lower neutral pH the sameEach 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
