Answered: What volume of 0.4 M Ba (OH)2 must be…

Science

Chemistry

What volume of 0.4 M Ba (OH)2 must be added to 50 mL of 0.3 M NaOH to give a solution 0.5 M in OH-.

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter8: Acids And Bases

Section: Chapter Questions

Problem 8.115P: 8-115 When a solution prepared by dissolving 0.125 g of an unknown diprotic acid in 25.0 mL of water...

See similar textbooks

Related questions

Q: What volume of (0.45 M) Ca(OH)2 must be added to 50 mL of 0.25-M (KOH) to give a solution 0.8 M in…

A: Concentration of Ca(OH)2 =0.45M Valume of KOH = 50ml Concentration of KOH =0.25M Concentration of…

Q: When 0.412 g of a weak base with Kb = 3.10 ×10-5 the base is dissolved in 1.00 L of solution, it has…

A: Assuming the molar mass is M Hence moles of base = mass / molar mass = 0.412 / M And concentration…

Q: (a) How many grams of NaOH are needed to neutralize20.0 mL of 0.150 M H2SO4 solution? (b) How many…

A: For the acid given, first we need to calculate number of moles, then the corresponding moles of…

Q: A buffer volution is prepared by adding s.50 g of ammonium chloride and o.0188 mol of ammonia to…

A: a. Given information: Mass of ammonium chloride NH4Cl or NH4+ =5.50 g The number of moles of ammonia…

Q: 2. A buffer solution of volume 0.500 L contains 1.68 g NH3 and 4.05 g (NH);SOu. a) What is the pH of…

A: “Since you have asked multiple questions, we will solve the first question [Q2] for you. If you want…

Q: Consider a buffer solution that consists of two separate components: the weak acid ch3coo aq), and…

A: In the given question, buffer of weak acid and its conjugate base is given i.e., CH3COOH and…

Q: 0.4723-g sample of primary-standard-grade Na2CO3 required 34.78 mL of an H2SO4 solution to reach the…

A: Given information: Mass of sample = 0.4723 g Volume = 34.78 mL

Q: ou dissolve 4.12 g of potassium formate (KCHO2) in sample water in the laboratory to make 322.00 mL…

Q: The pH of a saturated solution of Mg(OH)2 is 10.45. What is the pH of the solution after the…

A: Given-> pH of Mg(OH)2 = 10.45 Volume of HCl = 250.0 ml = 0.250 L (1L = 1000 ml) Molarity of HCl…

Q: How will the following sitations affect the final calculation of the molarity of HC2H3O2? The end…

A: Surpassing the end point of any titration is known as overshooting.

Q: How many milliliters of 0.0200 M Ca(OH)2are required to neutralize 94.8 mL of 0.0300 M HCI?

A: Here we are asked to calculate the volume 0.0200 M Ca(OH)2 that arerequired to neutralize 94.8 mL of…

Q: Example / What volume of 0.40 M Ba(OH)2 must be added to 50 mL of 0.30 M NAOH to give a solution…

A: Molarity of Ba(OH)2=0.40 M The volume of Ba(OH)2=y mL Molarity of NaOH= 0.30 M Volume of NaOH=50…

Q: 6) If 11.3 ml of 0.110 M HCI is required to neutralize 25.00 mL of a barium hydroxide solution, what…

Q: What is the volume (in mL) of 0.10 completely neutralize 25.00 mL ot according to the titration…

A: Answer

Q: Calculate the molarity of a NaOH solution if 24.50 mL of NaOH is titrated with 0.550 grams of KHP…

A: Number of moles for a given chemical species are defined as the ratio of mass to the molar mass.…

Q: Express the formality (F) the concentration of each of the following solutions: a. 28.4% NH3 by…

A: Given: % by weight of NH3 = 28.4 % Density of NH3 solution= 0.808 g/ml % by weight of HNO3= 69.5 %…

Q: A 15.0 mL solution of Ba(OH), is 2 neutralized with 29.0 mL of 0.200 M HCI. What is the…

A: We have to calculate the oxidation number of Carbon in C2O42- as follows in step 2:

Q: KHP I Trud 0.3130 9 16.72mL

A: For trial 1 Mass of KHP = 0.3130 g Molar mass(MM) KHP = 204.2 g Moles of KHP = mass/MM =…

Q: A 25.0 mL solution of HNO, is neutralized with 20.0 mL of 0.250 M Ba(OH)2. What is the concentration…

A: neutralisation reaction: Acid react with base to give salt and water In this reaction Ba(OH)2…

Q: Determin the cOH] concentration in o191 M MIOH)z soluhon, wher M is a compound. metal and M(O H)z is…

Q: A 10.00 Liter (L) sample of HCI requires 35L of 0.100 M KOH. What is the molarity (M) of the acid?

A: Given :- KOH + HCl → KCl + H2O Volume of HCl = 10.00 L Molarity of KOH solution = 0.100 M Volume…

Q: 4- Prepare 0.1 M of HCI in 100ml of distilled water from 6N of HCI?

A: Molarity of a solution is the number of moles of solute present in one liter of solution. It is…

Q: 5) Cal Culate the PH ofu solution which results from the mixing of 50.0ml of SM Hel which 5 omL of…

A: Given, the mixture of : 50.0mL of 0.3M HCl + 50.0 mL of 0.4M NH3. What is the pH of the resulting…

Q: What volume (in mL) of 0.28C HBr is required to neutralize 6 mL of 0.6000 M LIOH?

Q: Write a balanced chemical equation for the titration of an aqueous sample of NaHCO3 with HNO3. Be…

A: • We need to write a balanced chemical equation for the titration of an aqueous sample of NaHCO3…

Q: what volume of water would need to be added to 50.00 mL of 6.25*10^-2 M ALuminum hydroxide solution…

A: We know that aluminium hydroxide dissociates as : Al (OH) 3 --> Al 3+ + 3 OH - So, we can say…

Q: By titration, it is found that 14.7 mL of 0.190 M NaOH(aq) is needed to neutralize 25.0 mL of…

A: The neutralization reaction between NaOH and NaOH is as follows; NaOH + HCl → NaCl +…

Q: Solid potassium hydroxide is slowly added to 50.0 mL of a 0.329 M manganese(II) bromide solution…

A: According to the chemical equation, shown by equation (1), the number of mole of manganese(II)…

Q: What volume (mL) of 0.250 M HNO3 is required to titrate (neutralize) a solution containing 0.259 g…

A: Given : Mass of KOH = 0.259 g And Concentration of HNO3 = 0.250 M Molar mass of KOH = Atomic mass of…

Q: A 25.0 mL solution of HNO, is neutralized with 32.3 mL of 0.250 M Ba(OH)2. What is the concentration…

Q: Hydrocholic acid (13.5 mL of 0.235 M) is added to 431.0 mL of 0.0790 M Ba(OH)2 solution. what is the…

A: The moles of HCl and the Ba(OH)2 moles are first calculated. The balanced chemical equation is as…

Q: What

A: When temperature increases then solute solubility Increases in water because more and more Solute…

Q: A reaction requires the addition of 350.0 mL of a solution with a pH of 3.50. What mass of HNO3 (in…

A: pH :- The negative logarithm to the base 10 of hydrogen ion concentration of a solution expressed…

Q: What volume of 2.25M NaOH should be diluted with water to form 1.25 L of 1.50 M HCl?

A: M1 = 2.25 M M2 = 1.50 M V2 = 1.25 L

Q: If 37.23 mL of a sodium hydroxide solution is required to titrate 2.34 g of KHP, to the endpoint,…

A: Chemical reaction between sodium hydroxide and KHP is given by:

Q: How many milliliters of 0.2500M Ba(OH)2 must be added to 75.00ml of 0.3000N NaOH in order that the…

A: When a base with normality N1 and volume V1 is mixed with another base of normality N2 and volume V2…

Q: If 37.23 mL of a sodium hydroxide solution is required to titrate 2.34 g of KHP, to the endpoint,…

A: The reaction between NaOH and KHP is given below.

Q: What are the concentrations of ([H+], [OH-], [NH3+],[NH+4]) in the final solution when mixed 10mL of…

A: The concentration of the given species can be obtained by the balanced chemical reaction of NH3 with…

Q: What volume of 0.250 M KCl(aq) will completely react with 50.0 mL of 0.115M Pb(NO3)2(aq)?

A: We should equal equivalent of both KCl and Pb(NO3)2 to get volume of KCl Equivalent =…

Q: 3) what volume of 12M and 3M HCI must be Mixed to give 1lifer of 6M HCl

A: Answer:- This question is answered by using the simple concept of dilution equation which involves…

Q: By titration, it is found that 43.1 mL of 0.180 M NaOH(aq) is needed to neutralize 25.0 mL of…

Q: If it took 27.20 mL of 0.150 M NaOH to titrate 17.45 mL of an HCl solution, what is the molarity of…

A: Given: Concentration of NaOH = 0.150 M Volume of NaOH solution = 27.20 mL And volume of HCl solution…

Q: The pH for a solution with an [OH] of 1.0 x 10^-6 is?

A: We have Concentration of OH- as 10-6 , we have to predict the pH of Solution.

Q: 7. What volume of 0.120M NAOH will neutralize half of a 53.8 mL solution of 0.07 M propionic acid,…

A: Let the volume of NaOH is = V1 strength of NaOH is (S1)=0.120 M Volume of acid is (V2)=53.8/2=26.9ml…

Q: What volume of 0.386 M KOH, V, can be neutralized with 70.0 mL of 1.68 M HNO,? V =

A: KOH and HNO3 are strong base and strong acid respectively

Q: How many mL of 0.241 M Ba(OH)2 will react with 25.00 mL of 0.115 M HCI?

A: Given a question of Ba(OH)2 molarity of =0.241M1 -molarity of Hcl 0.115M2 reaction of complete…

Q: In a titration, 24.4 mLof a0.0154 Msolution ofBa (OH)₂ isneeded to neutralize20.0 mL of HCl. What…

A: Given, Ba(OH)2 solution: Concentration of Ba(OH)2 solution = 0.0154 M = 0.0154 mol/L Volume of…

Concept explainers

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.

Question

What volume of 0.4 M Ba (OH)₂must be added to 50 mL of 0.3 M NaOH to give a solution 0.5 M in OH^-.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

When 14.08 mL of 0.1594 M NaOH is added to 25.00 mL of 0.1235 M HX (an unknown weak acid), the resulting pH is 4.7. What is the Kaof the unknown acid?
10 mL of a solution of NaOH is found to be completely neutralized by 8 mL of a givensolution of HCl. If we take 20 mL of same solution of NaOH, the amount of HCl solution required to neutralize it will be:(a) 4 mL(b) 8 mL(c) 12 mL(d) 16 mL
(a) A 50.0 mL solution is prepared to be 1.29 M acetylsalicylic acid. In the first step, 8.55 mL of NaOH is titrated into the solution until the pH is exactly 5.0. What is the concentration of the titrant (NaOH)? (b) In the second step, enough 5.85 M nitric acid is added to the solution after the titration in part (a) is complete until the pH is one unit lower than the pKa of acetylsalicylic acid. What volume (mL) of nitric acid was added?
Determine the molar concentration of each ion present in the solutions that result from each of the following mixtures:(Disregard the concentration of H+ and OH- from water and assume that volumes are additive.) (a) 54.6 mL of 0.47 M NaCl and 77.6 mL of 1.16 M NaCl (b) 128 mL of 0.64 M HCl and 128 mL of 0.18 M HCl (c) 32.8 mL of 0.400 M Ba(NO3)2 and 24.8 mL of 0.258 M AgNO3 (d) 10.8 mL of 0.649 M NaCl and 21.7 mL of 0.177 M Ca(C2H3O2)2
Mg(OH)2 + Na2SO4 --> NaOH + MgSO4 Balance the equation. How many moles of NaOH is produced if 150mL of 1.5M Na2SO4 solution is used?
What mass of KHP will be completely neutrilized by 32.57 ml 0.175 M standard NaOH solution? The Molar Mass of KPH is 204.22 g/mol.
What volume of a 0.462 M NaOH solution would be required to titrate 2.85 g of pure KHP?
(a) How many grams of NaOH are needed to neutralize20.0 mL of 0.150 M H2SO4 solution? (b) How many litersof 0.500 M HCl(aq) are needed to react completely with0.100 mol of Pb1NO3221aq), forming a precipitate of PbCl21s)?
Determine the molar concentration of each ion present in the solutions that result from each of the following mixtures:(Disregard the concentration of H+ and OH- from water and assume that volumes are additive.) (a) 47.9 mL of 0.85 M HCl and 77.6 mL of 1.51 M HCl M H+= M Cl-= (b) 125 mL of 0.63 M CaCl2 and 125 mL of 0.22 M CaCl2 M Ca2+= M Cl-= (c) 31.0 mL of 0.333 M NaOH and 22.7 mL of 0.241 M HCl M Na+= M Cl-= M H+= M OH-= (d) 10.4 mL of 0.602 M H2SO4 and 21.5 mL of 0.151 M NaOH M Na+= M SO42-= M H+= M OH-=
55 ml of 1.5 M H C,H,CO, are used to titrate a sample of 0.87 M Ba(OH),- What is volume of the Ba(OH), used? 6.
4. How does the pH of each of the following solutions change when 5.0 mL of 1.0 M NaOH (a strong base) is added? Fill in the table. Give your answers with 2 decimals. Initial pH Final pH after adding NaOH Solution (a) 100.0 ml water (b) (c) 100.0 mL 0.150 M HNO2 (a weak acid) (Given: Ka = 4.5 × 10-4) 100.0 mL solution of 0.150 M HNO2 and 0.100 M NaNO₂
A 0.478 g sample of an unknown strong base is dissolved in 50.0 mL of water and titrated with a 0.135 M HCL solution. The equivalence point is reached when a total of 29.0 mL of HCL is added. The base and acid conbine in a 1:1 ratio. (a) How many moles of base are neutralized when the equivalent point is reached? (b) What was the initial concentration (M) of this unknown base? (c) What is the molar mass of the unknown base?