Homework Answers
PH of .01mM HCl is 5 , PH of .02M NaOH is 12.3.![1. Io 0.01 mer of her solution the concentration of H ion – 0.014 10 3 - 0.00001 M pH = -log [H0] =- log (0.0000) = 5 2. do 0](http://img.homeworklib.com/questions/79b8af00-9fd1-11ea-a44e-ddaa7d5fd4c9.png?x-oss-process=image/resize,w_560)
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can you help me with these
1. Calculate the pH of a 0.01 mM (1.0 mM...
Calculate the pH of the following solutions at 25 ℃ a) 1.0×10-5 M HCI c) 1.0×10-5...
Calculate the pH of the following solutions at 25 ℃ a) 1.0×10-5 M HCI c) 1.0×10-5 M NaOH Number Number pH b) 0.01 M HNO, d) 0.1 M KOH Number Numbero pH-
can someone please help me out with questions 1-5, please To add more information this was...
can someone please help me out with questions 1-5, please
To add more information this was given to me for a lab that used
a weak acid and we added a strong base through titration. We just
observed how the ph changes. Later we then used a buffer with a
weak acid to see how buffers affect ph change. These questions are
basically surrounded around those topics to help us prepare.
However, I'm kinda confused about answering them because weak...
anyone can help me with it...? biochemistry 2. A buffer contains 0.01 mole of lactic acid...
anyone can help me with it...? biochemistry
2. A buffer contains 0.01 mole of lactic acid (pKa-3.86) and 005 mole of sodium lactate per liter. (a) Calculate the pH of the buffer. (b) calculate the change in plH when 5 ml of 0.5 M HCl is added to 1L of the buffer. (c) what pll change would you expect if you added the same quantity of HCI to IL of pure water (8 points)?
Question 1 Calculate the pH of a 1.0 × 10−6M solution of HNO3 Question 2 Calculate...
Question 1 Calculate the pH of a 1.0 × 10−6M solution of HNO3 Question 2 Calculate the pH of a 1.0 × 10−1M solution of NaOH
Example 12. Calculate the pH of a 1.0 x 10-8 M solution of HCI. Calculate the...
Example 12. Calculate the pH of a 1.0 x 10-8 M solution of HCI. Calculate the pH of a 1.0 x 10-8 M solution of HCl. Calculate the pH of a 0.0500 M solution of the weak acid nitrous acid (pKa = 3.5).
Calculate the pH of each solution at 25 ∘C . 1.0×10−3 M HClpH= 0.01 M HNO3pH= 1.0×10−3 M NaOHpH= 0.1 M KOHpH=
Calculate the pH of each solution at 25 ∘C . 1.0×10−3 M HClpH= 0.01 M HNO3pH= 1.0×10−3 M NaOHpH= 0.1 M KOHpH=
Calculate the pH of each solution at 25 ∘C . 1.0×10−3 M HClpH= 0.01 M HNO3pH= 1.0×10−3 M NaOHpH= 0.1 M KOHpH=
Calculate the pH of each solution at 25 ∘C . 1.0×10−3 M HClpH= 0.01 M HNO3pH= 1.0×10−3 M NaOHpH= 0.1 M KOHpH=
need help with these questions please ISE 4: Neutralization You will need: 1 m/HCI 1 mil...
need help with these questions please
ISE 4: Neutralization You will need: 1 m/HCI 1 mil NaOH pH paper small graduated cylinder 50 ml beaker Write an equation for the dissociation of HCl in water. HCI - Na lootcrloo How many equivalents of Hare produced?_10 Write an equation for the dissociation of NaOH in water. How many equivalents of OH are produced? Co Will 5 mLs of 1.0 mM HCL neutralize 5 mLs of 1.0 mm NaOH? O Measure 5...
Please help, I'm so confused!!!! This is due wednesday night!!! i'm gonna fail :(((( pH of...
Please help, I'm so confused!!!! This is due wednesday night!!!
i'm gonna fail :((((
pH of Buffer Solutions Procedure: Acetic Acid-Sodium Acetate Buffer (pKa acetic acid = 4.75) Weigh about 3.5 g of Na2C2H302 3H2O, record the exact mass, and add to a 250 ml beaker. Measure exactly 8.8 mL of 3.0 M acetic acid (use 10 mL grad cylinder) and add to the beaker containing the sodium acetate. • Measure exactly 55.6 mL of distilled water and add to...
Calculate the [H^+], [OH^-], pH and pOH of the following solutions: a. 0.01 M HCl (aq)...
Calculate the [H^+], [OH^-], pH and pOH of the following solutions: a. 0.01 M HCl (aq) b. 0.02 M NaOH (aq)
Calculate the pH of the following solutions at 25 ℃ a) 1.0×10-5 M HCI c) 1.0×10-5 M NaOH Number Number pH b) 0.01 M HNO, d) 0.1 M KOH Number Numbero pH-
can someone please help me out with questions 1-5, please
To add more information this was given to me for a lab that used
a weak acid and we added a strong base through titration. We just
observed how the ph changes. Later we then used a buffer with a
weak acid to see how buffers affect ph change. These questions are
basically surrounded around those topics to help us prepare.
However, I'm kinda confused about answering them because weak...
anyone can help me with it...? biochemistry
2. A buffer contains 0.01 mole of lactic acid (pKa-3.86) and 005 mole of sodium lactate per liter. (a) Calculate the pH of the buffer. (b) calculate the change in plH when 5 ml of 0.5 M HCl is added to 1L of the buffer. (c) what pll change would you expect if you added the same quantity of HCI to IL of pure water (8 points)?
Example 12. Calculate the pH of a 1.0 x 10-8 M solution of HCI. Calculate the pH of a 1.0 x 10-8 M solution of HCl. Calculate the pH of a 0.0500 M solution of the weak acid nitrous acid (pKa = 3.5).
need help with these questions please
ISE 4: Neutralization You will need: 1 m/HCI 1 mil NaOH pH paper small graduated cylinder 50 ml beaker Write an equation for the dissociation of HCl in water. HCI - Na lootcrloo How many equivalents of Hare produced?_10 Write an equation for the dissociation of NaOH in water. How many equivalents of OH are produced? Co Will 5 mLs of 1.0 mM HCL neutralize 5 mLs of 1.0 mm NaOH? O Measure 5...
Please help, I'm so confused!!!! This is due wednesday night!!!
i'm gonna fail :((((
pH of Buffer Solutions Procedure: Acetic Acid-Sodium Acetate Buffer (pKa acetic acid = 4.75) Weigh about 3.5 g of Na2C2H302 3H2O, record the exact mass, and add to a 250 ml beaker. Measure exactly 8.8 mL of 3.0 M acetic acid (use 10 mL grad cylinder) and add to the beaker containing the sodium acetate. • Measure exactly 55.6 mL of distilled water and add to...
Calculate the [H^+], [OH^-], pH and pOH of the following solutions: a. 0.01 M HCl (aq) b. 0.02 M NaOH (aq)
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