Question

Part A.) 0.30 M HBr Express your answer using two decimal places. pH= Part B.) 3.5×10−4...

Part A.)

0.30 M HBr

Express your answer using two decimal places.

pH=

Part B.)

3.5×10−4 M KOH

Express your answer using two decimal places.

pH=

Part C.)

4.7×10−5 M Ca(OH)2

Express your answer using two decimal places.

pH=

Homework Answers

Answer #1

Part A.

0.30 M HBr

for strong acids,

pH = -log (conc. H+)

    = -log ( 0.3)

   pH = 0.52   ........... Answer

PART B

3.5×10−4 M KOH

[OH-]= 3.5 x 10^-4 M
pOH = - log (3.5 x 10^-4) = 3.46

pH = 14- pH

    = 14-3.46

   pH = 10.54   ................. Answer

PART C

4.7×10−5 M Ca(OH)2

[OH-]= 2 x 4.7 x 10^-5 = 9.4 x 10^-5 M ........... as Ca(OH)2 has 2 OH- ions
pOH = - log (9.4 x 10^-5) = 4.02

pH = 14 - 4.02

   pH = 9.98 ............. Answer

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Part A 7.6×10−3 M HBr, Express your answer using two decimal places. pH = Part B...
Part A 7.6×10−3 M HBr, Express your answer using two decimal places. pH = Part B 1.39 g of HNO3 in 550 mL of solution, Express your answer using three decimal places. pH = Part C 2.80 mL of 0.290 M HClO4 diluted to 55.0 mL , Express your answer using three decimal places. pH = Part D A solution formed by mixing 14.0 mL of 0.110 M HBr with 20.0 mL of 0.220 M HCl. Express your answer using...
Calculate the pH in 0.23 M HCO2H (Ka=1.8×10−4). Express your answer using two decimal places. pH...
Calculate the pH in 0.23 M HCO2H (Ka=1.8×10−4). Express your answer using two decimal places. pH = 2.20 SubmitMy AnswersGive Up Correct Part B Calculate the concentrations of all species present (HCO2H, HCO−2, H3O+, and OH−) in 0.23M HCO2H . Express your answers using two significant figures. Enter your answers numerically separated by commas. [HCO2H], [HCO−2], [H3O+],[OH−] =   M SubmitMy AnswersGive Up Part C Also calculate the percent dissociation. Express your answer using two significant figures.
Calculate the pH of each solution. Part A [OH−] = 6.8×10−11 M Express your answer using...
Calculate the pH of each solution. Part A [OH−] = 6.8×10−11 M Express your answer using two decimal places. Part B [OH−] = 3.6×10−3 M Express your answer using two decimal places. Part C [OH−] = 8.8×10−12 M Express your answer using two decimal places. Part D [OH−] = 9.4×10−4 M Express your answer using two decimal places.
Problem 16.45 Part A Calculate [OH−] for 1.0×10−3 M Sr(OH)2. Express your answer using two significant...
Problem 16.45 Part A Calculate [OH−] for 1.0×10−3 M Sr(OH)2. Express your answer using two significant figures. [OH−] = 2.0×10−3   M   SubmitMy AnswersGive Up Correct Part B Calculate pH for 1.0×10−3 M Sr(OH)2. Express your answer using two decimal places. pH = 11.30 SubmitMy AnswersGive Up Correct Part C Calculate [OH−] for 2.500 g of LiOH in 220.0 mL of solution. Express your answer using four significant figures. [OH−] = 0.4745   M   SubmitMy AnswersGive Up Correct Significant Figures Feedback: Your...
Part B Calculate the pH of a 0.10 M solution of barium hydroxide, Ba(OH)2. Express your...
Part B Calculate the pH of a 0.10 M solution of barium hydroxide, Ba(OH)2. Express your answer numerically using two decimal places. ph= Part C Calculate the pH of a 0.10 M solution of NaOH. Express your answer numerically using two decimal places. ph= Part D Calculate the pH of a 0.10 M solution of hydrazine, N2H4. Kb for hydrazine is 1.3×10−6. Express your answer numerically using two decimal places. ph= Part E Calculate the pH of a 0.10 M...
Please show answer and work! 0.15 M KCHO2 Express your answer to two decimal places. pH...
Please show answer and work! 0.15 M KCHO2 Express your answer to two decimal places. pH = Part B 0.15 M CH3NH3I Express your answer to two decimal places. pH = Part C 0.16 M KI, two decimal places and also find pH=
find pH - answers and work please 2.6×10−2 M HI Express your answer to two decimal...
find pH - answers and work please 2.6×10−2 M HI Express your answer to two decimal places. pH = SubmitMy AnswersGive Up Part B 0.117 M HClO4 Express your answer to three decimal places. pH = SubmitMy AnswersGive Up Part C a solution that is 5.2×10−2 M in HClO4 and 2.8×10−2 M in HCl Express your answer to two decimal places. pH = SubmitMy AnswersGive Up Part D a solution that is 1.90% HCl by mass (Assume a density of...
Calculate the pH of the following solutions: 1. 0.060 M HClO4   Express your answer using two...
Calculate the pH of the following solutions: 1. 0.060 M HClO4   Express your answer using two decimal places. 2. 2.3 M HCl   Express your answer using two decimal places. 3. 1.1 M KOH   Express your answer using two decimal places. 4. 0.080 M NaOH   Express your answer using two decimal places.
Find the PH 8.0×10−2 M RbOH and 0.130 MNaHCO3 Express your answer using two decimal places.
Find the PH 8.0×10−2 M RbOH and 0.130 MNaHCO3 Express your answer using two decimal places.
Problem 16.45 part 2 Part E Calculate [OH−] for 1.60 mL of 0.130 M NaOH diluted...
Problem 16.45 part 2 Part E Calculate [OH−] for 1.60 mL of 0.130 M NaOH diluted to 1.50 L . Express your answer using three significant figures. [OH−] =   M   SubmitMy AnswersGive Up Part F Calculate pH for 1.60 mL of 0.130 M NaOH diluted to 1.50 L . Express your answer using three decimal places. pH = SubmitMy AnswersGive Up Part G Calculate [OH−] for a solution formed by adding 4.70 mL of 0.150 M KOH to 20.0 mL...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT