You have chosen Methylamine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.48 M in this salt. The desired pH of the buffer should be equal to 9.75. To prepare the buffer, a total volume of 550 mL is required. The stock solution of the weak base is available at 1 gallon with a concentration of 0.98 M. (Remember the lesson on dilution: C1V1=C2V2) 4. How many mL should be taken from the stock solution to prepare the desired buffer solution? (round off final answer to 1 decimal place)

Q: Calculate the pH of 50.00 ml distilled water after the addition of 4.00 ml 0.10 M HCl. 2. Calculate…

A: Given the volume of distilled water = 50.00 mL Volume of 0.10 M HCl added = 4.00 mL * (1L/1000 mL) =…

Q: explain why the pH of a buffer solution remains unchanged even if we add a little base.

A: Buffer solution: The buffer solution is an aqueous solution consisting of a mixture of a weak acid…

Q: pH = 6.9 small can be neutralized can not be neutralized is not dissolved large Reset Help When…

A: Buffer solution — A solution which prevents change in pH on adding small amount of any acid or base…

Q: If your lab partner misread the concentration of the sodium hydroxide solution and recorded a number…

A: Given: Lab partner misread the concentration of NaOH solution and recorded a number that was too…

Q: Which theory or concept can explain buffer solution precisely? Explain your answer.

A: a buffer solution is formed by mixture of weak acid and its conjugate base or weak base and its…

Q: Determine if true or false: 1) ionic compounds, that dissolve well in water, and strong acids are…

A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: A buffer solution contains 0.457 M ammonium bromide and 0.335 M ammonia. If 0.0430 moles of sodium…

A:

Q: A 10.0 mL solution of 0.540 M NH, is titrated with a 0.180 M HCl solution. Calculate the pH after…

A: The objective of this question is to calculate the pH of a solution of NH3 after the addition of…

Q: A student must make a buffer solution with a pH of 2.00. Determine which weak acid is the best…

A: A buffer works best at a pH closer to the pKa value of the acid. Closer the pKa value of the acid to…

Q: In titrating 40.0 mL of 0.10M of HCI solution with 0.15 M of KOH solution, what would be the pH of…

A: Given that ,  HCl (acid) KOH (base) Molarity(Ma) = 0.10 M Molarity (Mb) = 0.15 M Volume (Va)…

Q: Use the References to access important values if needed for this question. A buffer solution…

A:

Q: Answer the following questions about the titration curve shown below. a) Choose the correct words…

A: (a) The sample is weak acid because initial pH is near to 3.  The titrant is strong base.  pH at…

Q: The titration of 50.00 mL of 0.150-M HCl with 0.150-M NaOH (the titrant) is carried out in a…

A: The balanced equation for the reaction between HCl and NaOH is   HCl + NaOH --------> NaCl + H2O…

Q: you need to prepare a pH = 9.20 buffer solution containing NH3 and NH4Cl. if you start with 0.52 M…

A:

Q: In general, adding a strong acid or a strong base to a buffer solution _________ neutralizes the…

A: Buffer solution is the solution which resist change in pH on addition of small amount of acid or…

Q: An analytical chemist is titrating 88.9 mL of a 0.2700M solution of ammonia (NH3) with a 0.4900M…

A: Ammonia, NH3(aq) is a monoacidic weak base with pKb = 4.74 HIO3(aq) is a monoprotic strong acid.…

Q: A pH buffer is a solution that resists changes in pH when acids or bases are added to it—typically,…

A: We have to prepare 7.00 L of pH = 12.00 buffer.

Q: The final volume of buffer solution must be 100.00 mL and the final concentration of the weak acid…

A: In the above question given that -  Final volume of buffer solution =100.00 ml  Final concentration…

Q: I don't know if it is possible, but I have to make a solution of acetic acid with a pH of 4 and a…

A: Required pH of Acetic acid solution  =  4 Volume of acetic acid solution required = 250 mL Volume of…

Q: Which of the following combinations of chemicals makes a buffer? Mark all that apply. (Identifying…

A:

Q: A sample containing 26.38 mL of 0.1439 M HBr is titrated with a solution of NaOH having a molarity…

A: pH is defined as the negative logarithm of hydronium ions. pH value ranges from 0 to 14. 0 is very…

Q: Using the table of the weak base below, you have chosen Methylamine as your weak base in the buffer…

A:

Q: in titrating 40.0 mL of 0.10 M of HCI solution with 0.15 M of KOH solution, what would be the pH of…

A: The balanced chemical reaction is  HCl + NaOH ------> NaCl + H2O Number mmoles of HCl = molarity…

Q: Explain the difference between a buffered and an unbuffered solution. How does the pH of an…

A: Buffer solution: A buffer is a solution of weak acid and conjugate base or weak base and conjugate…

Q: Comment on the shape of your graph. Thoroughly explain the chemical cause of each flat or steep…

A: The titration curve is a graph of the volume of titrant,  plotted against the pH.

Q: A few small drops of water are left in a burette that is used to titrate a base into an acid…

A: If the acid concentration is low then it will not affect too much since small amount of water will…

Q: Consider a solution that initially contains 0.40 mol fluoride anion and 0.30 mol of hydrogen…

A: Given information,         A solution that initially contains 0.40 mol fluoride anion and 0.30 mol…

Q: A buffer solution is prepared by combining 0.898 moles of formic acid and 0.733 moles of sodium…

A: The buffer solution is prepared by mixing with 0.898 moles of formic acid and 0.733 moles of sodium…

Q: ffer solution is prepared by combining 0.848 moles of formic acid and 0.719 moles of sodium formate.…

A: Mole  formic acid= 0.848    Mole sodium formate = 0.719  Mole of NaOH = 0.126  Ka = 1.8×10-4.   Pka=…

Q: 5 A buffer system is prepared by combining 0.569 moles of ammonium chloride (NH4CI) and 0.586 moles…

A: A buffer is a solution which resist any change in pH on adding a small amount of acid or base . it…

Q: A 10.0 mL solution of 0.330 M NH, is titrated with a 0.110 M HCI solution. Calculate the pH after…

A: Given,  Molarity of NH3 = 0.330 M Volume of NH3 = 10.0 mL Molarity of HCl = 0.110 M.  Volumes of HCl…

Q: Suppose 90.00 ml of 0.200M HCI is added to an acetate buffer prepared by dissolving 0.100 mol of…

A: Volume of HCl = 90.00 mLConcentration of HCl = 0.200 MNumber of moles of acetic acid = 0.100…

Q: When pH titrations occur, more data points become necessary at the vertical deflection near the…

A: Solution - According to the question - Given - In this given graph we assume this is a titration…

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.