50 mL of a wastewater sample needs 21 mL of 0.1 M hydrochloric acid, HCI (MW = 36.5) to reduce its pH to one unit. Calculate buffer capacity for the wastewater in mg HCI/L.
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- A 0.2386-g sample contained only NaCl and KBr was dissolved in water and required 50.00 mL of 0.04500 M AgNO3 for complete titration of both halides. If we assume there is x mol of NaCl in the original sample, which of the following statements are CORRECT? There are multiple correct answers. MW(NaCl) = 58.44 g/mol. MW(KBr) = 119.002 g/mol. There is x mol of KBr in the original sample. x+(0.2386-58.44x)/119.002-50.00*0.04500 There is (0.002250 - x) mol of KBr in the original sample. 58.44x+119.002(0.002250-x)=0.23861: Cônsider the following buffer solution: 600.0 ml 0.550 M CH,COOH 0.325 M NACH,CO K - 1.76 x 10 Determine the pH of the buffering system after 170.0 ml of 2.00 M NaOH has been added. Part "A": Process the initial information and determine the buffer's initial pH and the initial moles of CH;COOH, NACH,CO0 and NAOH. Part "B": Analyze the in information above and determine if this is a Type I, Il or III Bothering the Buffer problem. Explain your decision (.a sentence or two should be sufficient) Part "C": Perform the necessary calculations and determine the pH of the buffer after the NAOH addition. Your answer should contain the correct number of S.F. Part "D": Compare your answer to the buffer's original pH and determine whether it is reasonable or not. Explain your rationale. O Focus 中Please help me...... a. Do you expect the pH at the equivalence to be lowest when a 0.0500 M (CH3)3N(aq) solution or a C5H5N(aq) solution is titrated with a 0.0500 M HCl(aq) solution at 25.0 oC? Motivate your answer! (CH3)3N (Kb = 6.5 × 10-5) and C5H5N (Kb = 1.7×10-9) are weak monoprotic bases. Calculate the pH at the equivalence point and 25 oC when 1.00 L of a 0.0500 M C5H5N(aq) solution is titrated with a 0.0500 M HCl(aq) solution. Calculate the molar solubility for CaCO3 in a 0.060 M Ca(NO3)2(aq) solution. Ksp= 3.1 × 10-9 for CaCO3.
- A chemistry graduate student is given 250. mL of a 1.40M ammonia (NH3) solution. Ammonia is a weak base with K-1.8x10 should the student dissolve in the NH3 solution to turn it into a buffer with pH = 9.17? What mass of NH, Br You may assume that the volume of the solution doesn't change when the NH4Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. ?A chemistry graduate student is given 300. mL of a 1.60M pyridine (C H,N) solution. Pyridine is a weak base with K,=1.7 × 10 What mass of CH,NHC1 should the student dissolve in the CH,N solution to turn it into a buffer with pH = 5.16? You may assume that the volume of the solution doesn't change when the CH,NHCI is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.You prepare a buffer solution by dissolving 2.00 g each of benzoic acid (HC7H5O2, MW = 122.12) and sodium benzoate (NaC7H5O2, MW = 144.10) in 750.0 mL of water. The pKb of sodium benzoate is 9.80. What is the pH of this buffer solution? [Assume no volume change.]
- A student titrates an unknown weak acid, HA, to a pale pink phenolphthalein endpoint with 25.0 mL of 0.100 M NAOH. The student then titrates in 13.0 mL of 0.100 M HCI to the solution containing the neutralized unknown acid (HCI was delivered from a second buret). The pH of the resulting solution is pH = 4.7 (the solution after the HCI has been added). Which of the following statements is true? The pka of the acid is 4.7. At pH = 4.7, half of the conjugate base, A¯, has been converted to HA. The pka of the acid is less than 4.7. More than one of these statements is correct. The pka of the acid is greater than 4.7. To|0|0|0< A buffer solution that is 0.401 M in HF and 0.401 M in KF has a pH of 3.14. The addition of 0.01 mol of H3O+ to 1.0 L of this buffer would cause the pH to A C The capacity of this buffer for added H₂Ot could be increased by the addition of 0.159 molA 0.7500-g sample of pure KHP (Fwt=204.2g/mol) was dissolved and titrated with 35.0 mL of NaOH. The end point was overstepped and it was necessary to backtitrate with 3.50 mL HCl. Calculate the molarity of NaOH and HCl if the ratio is 30.0 mL NaOH to 25.0 mL HCl. Approximately 6 mL of conc.perchloric acid ( 72% ) was transferred to a bottle and diluted with about 1 liter of water. A sample containing 251.5 mg of primary standard Na2B4O7.10H2O required 27.41 mL of the HClO4 solution to reach the methyl red end point. What is the molar concentration of the HClO4 solution? (Fwt.= 382g/mol) Na2B4O7.10H2O + HClO4 ------------> NaClO4 H2B4O7.10H2O A 1.900-g sample is analyzed for benzoic acid content. The sample was dissolved and diluted to the mark using a 500-mL volumetric flask. A 30.0mL aliquot required 5.00mL of 0.1575M NaOH solution. Calculate the %(w/w) benzoic acid (Fwt=122) in the sample.…
- A chemistry graduate student is given 500. mL of a 1.80M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K,= 4.9 x 10 – 10 What mass of KCN should the student dissolve in the HCN solution to turn it into a buffer with pH =9.70? You may assume that the volume of the solution doesn't change when the KCN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 国 国 回A chemistry graduate student is given 300. mL of a 0.90M ammonia (NH,) solution. Ammonia is a weak base with K,=1.8 × 10 ° 5 What mass of NH,Br should the student dissolve in the NH, solution to turn it into a buffer with pH = 8.92? %3D You may assume that the volume of the solution doesn't change when the NH,Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. x10The pK, value for HF is 3.14. Would a buffer prepared from HF and NaF with a pH of 1.14 be considered to be an effective buffer? A buffer in which the mole ratio of NaF to HF is 0.46 has a pH of 2.80. Would this buffer solution have a greater capacity fo added acid ( H3O*) or added base ( OH )? A buffer solution that is 0.425 M in CH, COOH and 0.425 M in CH3 COONA has a pH of 4.74. 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 H30 could be increased by the addition of 0.130 mol