What mass of solid K₂CO3 (molar mass = 138.0 g/mol) should be added to 0.995 L of 0.535 M HCO3 to make a buffer with a pH of 10.32? (pKa of HCO3 = 10.32)
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- A buffer is made up of equal volumes (513.8 mL of each) of 0.846 M A H and 0.845 M A minus. 15.54 mL of 0.404 M N a O H is added to the buffer. How many moles of A H are present after the addition of N a O H? Please use correct significant figures. Answer: 0.428 MCalculate the pH of a NH4*/NH3 buffer that was prepared with 100.0 mL of 0.500 M NH4CI and 50.0 mL of 0.400 M NH3 solution. (K, for NH3 is 1.76x10-5) Answer:What is the buffer range for the buffer made from mixing 70.0 mL of 0.15 M HCIO with 25.0 mL 0.20 M KCIO? Ka of HCIO = 2.9 × 10-8 A) pH 7.46 to pH 5.46 B) pH 8.86 to pH 6.86 C) pH 8.54 to pH 6.54 D) pH 8.22 to pH 6.22 E) None of these
- How many grams of solid ammonium chloride should be added to 2.00 L ofa 5.44x10 M ammonia solution to prepare a buffer with a pH of 8.340? grams ammonium chloride - 8- Submit Answer Retry Entire Group 4 more group attempts remainingA buffer solution that is 0.471 M in HCN and 0.471 M in NaCN has a pH of 9.40. The addition of 0.01 mol of OH to 1.0 L of this buffer would cause the pH to The capacity of this buffer for added OH could be increased by the addition of 0.150 mol of the weak acid of the salt Submit Anawer Retry Entre Group 9 more group attempta remalningYou need to prepare 100.0 mL of a pli 4.00 buffer solution using (0.100 M henzoic acid (pk, = 4.20) and 0.160 M sodium benzoate. %3D How many milliliters of eaclh solution should be mixed to prepare this buffer? henzoic acid: sodium benzOute: mL ml.
- How many grams of solid sodium cyanide should be added to 1.50 L of a 0.161 M hydrocyanic acid solution to prepare a buffer with a pH of 9.903? (K₁ (HCN) = 4.00 x 10-¹0) a Mass= g Retry Entire Group Submit Answer 9 more group attempts remaining Previous Next%3D What mass of NaOH does this butffer neutralize before the pH rises above 4.00? ( K. (HF) =3.5 x 10) Express your answer in grams to two significant figures. A 340.0 ml buffer solution is 0.140 M in HF and 0 140 M in NaF m- 3.1 Submit Previous Answers Beauest Answer X Incorrect; Try Again; 2 attempts remaining Part B If the same volume of the buffer was 0.360 M in HF and 0.360 M in NaF, what mass of NaOH is neutralized before the pH rises above 4.00? Express your answer in grams to two significant figures. m- 8.04Which of the following chemicals would be the best buffer for a pH 9.00 solution: NH3 (Kb = 1.75x10-5), C6H5NH2 (Kb = 3.99x10-10), H2NNH2 (Kb = 3.00x10-6), C5H5N (Kb = 1.69x10-9)? A) H2NNH2 B) C6H5NH2 C) NH3 D) C5H5N
- Vomnting irom Smo... 2 Cannabinoid Hyper. Video: Deep muscle.. Question 3 of 5 How many moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer with a pH of 2.90? (Ka for HF is 6.8 x 10 4) 0.13 mol 4. 8. 9. +/- 0. 68 P Type here to search 3. LO 近A laboratory manager wants to prepare 500.00 mL of a buffer with a pH of 4.471 from equimolar solutions of CH3CO2H (Ka = 1.800e-5) and LiCH3CO2. What volume of the LiCH3CO2 solution would be required? Key Concept: Buffers resist pH change and are prepared by mixing the conjugate acid and base together. The pH is determined from the Henderson-Hasselbach equation: pH = pKa + log([A−]/[HA]).Solution: Since the molarities of the two solutions making the buffer are the same, the Henderson-Hasselbach equation can be written as: pH = pKa + log(V(A−)/V(HA)) where V(A−) = the volume of the conjugate base and V(HA) = the volume of the conjugate acid.✓ Saved Question 26 [F] To make a buffer from a mixture of HF and NaF that has a pH = 3.35 what must the ratio of K, be? K₂ for HF = 7.2 x 10-4. [HF] Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. 2.5E5 for 2.5 x 10*) Typed numeric answer will be automatically saved.