Calculate the PH
1.) 9.55×10−2 M HBr
2.) 1.28×10−3 M KOH
3.) 8.89×10−3 M HNO3
4.) 2.54×10−4 M Sr(OH)2
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Calculate the PH 1.) 9.55×10−2 M HBr 2.) 1.28×10−3 M KOH 3.) 8.89×10−3 M HNO3 4.)...
Calculate the pH of each solution. A. 7.55×10−2 M HBr B. 6.28×10−3 M KOH C. 1.89×10−3 M HNO3 D. 5.54×10−4 M Sr(OH)2 E. [OH−] = 9.9×10−7 M F. [OH−] = 8.6×10−8 M G. [OH−] = 9.2×10−11 M H. [OH−] = 3.4×10−2 M
Calculate the pH of each of the following solutions. 0.50 M HBr 3.1×10−4 M KOH 4.2×10−5 M Ca(OH)2
1) A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 16.0 mL of KOH.Express your answer numerically. pH=_______ 2) A 75.0-mL volume of 0.200 M NH3 (Kb = 1.8 x10-5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 13.0 mL of HNO3.Express your answer numerically. pH=_______ 3) A 52.0-mL volume of 0.35 M CH3COOH (Ka = 1.8 x10-5 ) is titrated with 0.40 M NaOH. Calculate...
Calculate [OH -] and pH for each of the following solutions. (a) 0.0061 M KOH [OH-] = ? M pH=? (b) 0.0225 g of KOH in 540.0 mL of solution [OH-] = ? M pH=? (c) 53.0 mL of 0.00788 M Sr(OH)2 diluted to 700 mL [OH-] = ? M pH=? (d) A solution formed by mixing 44.0 mL of 0.000590 M Sr(OH)2 with 25.0 mL of 3.2 x 10-3 M KOH [OH-] = ? M pH=? Calculate [OH-] and...
A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 12.0 mL of KOH. Express your answer numerically. A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 13.0 mL of HNO3. Express your answer numerically. A 52.0-mL volume of 0.35 M CH3COOH (Ka=1.8×10−5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 33.0 mL...
A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 15.0 mL of KOH. Express your answer numerically. pH = SubmitHintsMy AnswersGive UpReview Part Part C A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 27.0 mL of HNO3. Express your answer numerically. pH = SubmitHintsMy AnswersGive UpReview Part Part D A 52.0-mL volume of 0.35 M CH3COOH...
A: 48.0 mL volume of 0.25 M HBr is titrated with 0.50 M KOH. Calculate the pH after addition of 24.0 mL of KOH at 25 ∘C B: Consider the titration of 50.0 mL of 0.20 M NH3 (Kb=1.8×10−5) with 0.20 M HNO3. Calculate the pH after addition of 50.0 mL of the titrant at 25 ∘C. C: A 30.0-mL volume of 0.50 M CH3COOH (Ka=1.8×10−5) was titrated with 0.50 M NaOH. Calculate the pH after addition of 30.0 mL of NaOH at 25...
1.) A 80.0mL volume of 0.25 M HBr is titrated with 0.50 M KOH. Calculate the pH after addition of 40.0mL of KOH. 2.) Consider the titration of 50.0 mL of 0.20 M NH3 (Kb=1.8
Part B A 72.0 mL volume of 0.25 M HBr is titrated with 0.50 M KOH. Calculate the pH after addition of 36.0 mL of KOH at 25 ∘C. Express the pH numerically. Part C Consider the titration of 50.0 mL of 0.20 M NH3 (Kb=1.8×10−5) with 0.20 M HNO3. Calculate the pH after addition of 50.0 mL of the titrant at 25 ∘C. Express the pH numerically. Part D A 30.0-mL volume of 0.50 M CH3COOH (Ka=1.8×10−5) was titrated with 0.50 M NaOH. Calculate the...
Part B A 96.0 mL volume of 0.25 M HBr is titrated with 0.50 M KOH. Calculate the pH after addition of 48.0 mL of KOH at 25 ∘C. Express the pH numerically. Part C Consider the titration of 50.0 mL of 0.20 M NH3 (Kb=1.8×10−5) with 0.20 M HNO3. Calculate the pH after addition of 50.0 mL of the titrant at 25 ∘C. Express the pH numerically. Part D A 30.0-mL volume of 0.50 M CH3COOH (Ka=1.8×10−5) was titrated with 0.50 M NaOH. Calculate...