Calculate the pH of solution made by combining 100 ml of 0.28 М НС,Н;0; and 50 ml of 0.36 M NaOH, Ka for HС-Н,О,31.8 х 10_5

Q: 38. What is the molar solubility of Ag.PO, in pure water? a) 8.89 x 10¹ mol L b) 9.43 x 10 mol Lª c)…

A: Since you have posted multiple questions, we will provide the solution only to the first question as…

Q: In the acid base titration by using 2.5 M of hydrochloric acid solution . the reading of burette…

A: Given that ,  Concentration of HCl (M1) = 2.5 M  Volume of HCl (V1) = 8 ml Volume of NaOH (V2) = 2…

Q: Vithout doing detailed calculations, determine which of the following will raise the pH when added…

A: SOLUTION: Step 1: The first solution is the buffer solution of NH3 and NH4OH. In the second case the…

Q: What mass of the salt, N a A would you have to added to 0.10 M H A (weak acid) with a volume of 127…

A: The weak acid (HA) and the salt (NaA) forms an acidic buffer whose pH is given by the expression:…

Q: An aqueous solution is prepared to be 0.232 M in sodium nitrite and 0.101 M in acetic acid. (1) Is…

A: An aqueous solution is prepared to be 0.232 M in sodium nitrite and 0.101 M in acetic acid. 1) Is…

Q: 3 mL of HCI is titrated with 0.2 M NaOH and 3 mL NaOH is consumed. What is the concentration of 10…

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Q: For a solution of 2.5 M H2CO3 (Ka = 4.4 x 10-7), calculate: (a) [H*] (Ь) рH (c) percent ionization

A: Given: Concentration of H2CO3 = 2.5 M Ka1 = 4.4×10-7 Ka2 = 4.8×10-11

Q: 1. The mixture of anions is an effective blood buffer with the following acid-base equilibrium: HO"…

A: According to Le Chatelier's principle if concentration of reactants or products of a chemical…

Q: What is the pH if 0.188 L of 0.206 M KOH is added to the solution be?

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Q: ralence point. Gi nt (in grams) of t 5738

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Q: he ammonia – ammonium chloride buffer keep the pH: а. above 14; below 7; с. above 7 O d. =7

A: The correct answer about ammoniacal buffer is given below

Q: Calculate the pOH after addition of 15.66 mL of 0.1621 M HBr to 25.00 mL of 0.1546 M CH3NH2.…

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Q: 5. An Indicator Molecule Br Br OH HO, -Br Br = 4.89 pK. Yellow pH 5.5 Shown above is a molecule…

A: The given molecule is an acid-base indicator.

Q: H.W 1- Calculate the pH of 2 solution prepared by adding 25 ml of 0.IM of NAOH solu. to 30 ml of…

A: NaOH+CH3COOH→CH3COONa+H2O0.025L     0.030L0.1M         0.2MNo. of moles of NaOH=0.025×0.1M=0.0025No.…

Q: [References) Given a 1.00 L solution that is 0.60 M HF and 1.00 M KF, calculate the pH after 0.10…

A: Given that : Volume = 1 L Molarity of HF = 0.60 M Molarity of KF = 1.00 M To calculate pH after…

Q: A 25.0 mL sample of a saturated C a ( O H ) 2 solution is titrated with 0.026 M H C l , and the…

A: Information about the question

Q: 4. 20.0 mL of 0.200 M CH3COOH is titrated with 0.100 M NaOH. a) What volume of NaOH is necessary to…

A: Given-> Volume of CH3COOH = 20.0 ml Molarity of CH3COOH = 0.200 M Molarity of NaOH = 0.100 M

Q: oi ("muinoans

A: mmoles of NaOH = ( 0.10 • V )mmol  mmoles of HF = ( 20 • 0.10 ) = 2mmol  mmoles of Salt = mmoles of…

Q: Which of the following pairs of substances can be used to make a buffer solution? O a. NH3 &…

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

Q: 4. Which of the three sulutions (water, 0.IM buffer,0.0IM buffer) was besi able to conirol the pH…

A: Given solutions: Water, 0.1 M buffer, 0.01 M buffer

Q: [Review Topics] [Reterences] Use the References to access important values if needed for this…

A: The question is based on the concept of solubility product Principle.   it states that a weak…

Q: A- Calculate the pH of the resulting salt solution, when 100 ml of 0.1IN (HCI) was added to 0.IN…

A: The balanced chemical equation for the reaction of HCl and NH3 is                      NH3…

Q: Drawing Conclusions 1. How are O.010 M solutions of HCI, CHOOH, and CH,COOH similar to one another…

A: Concentration of a solution describe the nature of its reactivity and quantity of its solute and…

Q: 1). The sample of 25.00 mL of 0.010 M HCOOH is titrated with 0.020 M KOH. (a) Show the reaction…

A: Since you have asked question with multiple subpart, we will solve the first  three subpart question…

Q: 1. Complete the table with suitable calculation. 2. Construct a suitable reaction for the above…

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Q: 2) How many moles of methylammonium chloride (CH;NH;Cl) are needed to prepare a buffer that is pH…

A: Given- pH of buffer = 9.64 Moles of methylamine CH3NH2 = 0.15 pKb CH3NH2 = 3.36 To find- Moles of…

Q: Which one of the following solutions is not a buffer solution? O HF/NaF HBr/NaBr O NH3/NH.CI…

A: Among those the one that won't be considered as buffer is given below

Q: 2) How many moles of methylammonium chloride (CH;NH;CI) are needed to prepare a buffer that is pH…

A: Given, Moles of CH3NH2 (base) = 0.15 mol Moles of CH3NH3Cl (salt) = x = ? pH = 9.64 pKb = 3.36

Q: Part A A 1.0 L buffer solution is 0.250 M HC,H3O, and 0.040 M NaC,H3O,. Which of the following…

A: 6

Q: IReview Topies] (Reterences) Use the References to access important values if needed for this…

A: pH change =? pH change = pH after Addition - pH before addition Number of Mol of KOH = 0.124 mol […

Q: 1. Write a balanced equation for each of the following neutralization reactions a HSO, and RBOH H2…

A:

Q: (c) after adding 0.030 mol of HCI to 1.0 L of the buffer solution in part (a) 0.030тol [H;O*]added…

A: Solution: Here we have acetate buffer solution. We have added 0.030 mole of HCl and need to find out…

Q: Determine the pH of a buffer formed by dissolving 20.0 g NaCH:COO into a 500.0 mL solution of 0.150…

A: The molarity of acetic acid is 0.150 M. The amount of sodium acetate added to 500.mL of solution is…

Q: I titrate a sample of aqueous sulfuric acid with 14.27mL and 0.117M Potassium hydroxide. Calculate…

A:

Q: Q2: Calculate the pH of the following acid-base buffers. 100 ml. of 0.025 M formic acid and 0.015 M…

A: pH of buffer Using Hendersen-Hasselbalck equation,  pH= pKa + log(base/acid)  [formic acid] (acid) =…

Q: If 50.00 ml of 1.00M HC,H,O; (K, = 1.8 x 10*) is titrated with 1.00 M NaOH. What is the pH of the…

A: Volume of CH3COOH = 50ml Concentration of CH3COOH = 1M Concentration of NaOH = 1M Ka = 1.8×10-5 We…

Q: a. Calculate the number of moles of HCI(g) that must be added to 1.0 L of 1.1 M NaC,H3O2 to produce…

A:

Q: what volume of 13,4 H ammonia (NH3) must be added to 250.0m) of 0.850 M HNO3 to form a buffer wi th…

A: Basic-buffers are made-up of weak base. Their solution contains this base together with a salt…

Q: Q2: Draw (p) the titration curve ( ) when you add (0, 15, 40 and 50 ml) of 0.1M NaOH to 40ml of 0.1M…

A: A titration curve is drawn by plotting pH of solution on Y-axis and volume of titrant, NaOH on…

Q: 16. For 1.0 M of the following solution, which chemical gives the highest pH value? (A) NaF (B)…

A: For the highest pH value . We know in pH scale the value of pH increases from lest to right i.e. as…

Q: Calculate the [Y"] in a saturated solution of YF3 in 0.003150 M NaF(). (Kap for YF3 = 8.6 x 10") %3!

A: Solubility product (Ksp) is defined as the products of ions present in a solution of a salt.

Q: Determine the mass of solid NaCH,COO that must be dissolved in an existing 500.0 mL solution of…

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

Q: 13.) The ha ft firmic acid CHCO, H) is 1.8x10-4. pH g a frmate "(Na HCO2)? Unt is tje pH qa O.35M…

A:

Q: 5. A 25.00-ml portion of a H₂SO, solution was titrated with a 0.256 M KOH solution. To reach the…

A:

Q: Question 4 a) Determine the pH of 0.10 M NAOH solution. b) Find out the pH of a 0.002 M acetic acid…

A: Question   4  a)  Concentration of NaOH = 0.10 M    NaOH is a strong base and will be completely…

Q: How many milliteters CmL) of 1.0M Na OH woruld be needed to neutralize and precipitate 20.0L oh…

A: Acid reacts with base to form salt and water. This reaction is known as neutralization reaction. So,…

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.