1) A 25.00 mL sample of unknown concentration of HNO3 solution requires 22.62 mL of 0.02000 M NaOH to reach the equivalence point. What is the concentration of the unknown HNO3 solution?
Q: What volume (in mL) of 0.2300 M HBr is required to neutralize 50.00 mL of 0.7000M KOH?
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Q: A 30.0 mL solution of LiOH is neutralized with 38.0 mL of 0.150 M HBr. What is the concentration of…
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Q: If 0.3041 g of a diprotic solid acid is neutralized by 35.45 mL of 0.0997 M NaOH, calculate the…
A: Given, 0.3041 g of a diprotic solid acid 35.45 mL of 0.0997 M NaOH
Q: What is the molarity of a nitric acid solution if 43.33 mL of 0.1000M KOH solution is needed to…
A: Balanced chemical equation: HNO3 + KOH → KNO3 + H2O By stoichiometry of reaction: Moles of…
Q: What volume (in mL) of 0.2750 M HCl is required to neutralize 50.00 mL of 0.8000 M NaOH?
A: Given data,Molarity of HCl=0.2750MMolarity of NaOH=0.800MVolume of NaOH=50.0mL
Q: 10 mL of a solution of NaOH is found to be completely neutralized by 8 mL of a givensolution of HCl.…
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Q: A 15.0 mL solution of Ba(OH)2 is neutralized with 30.5 mL of 0.200 M HCI. What is the concentration…
A: . For acid-base neutralization reaction . Number of gram equivalent of acid = Number of gram…
Q: A. If 24.37 mL of 0.5183 M sodium hydroxide are required to exactly neutralize 15.79 mL of oxalic…
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Q: concentration
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Q: 33.82 ml of an HNO, solution of unknown molarity requires 29,95 ml of 0.100M NaOH solution to be…
A: Let M1 is the molarity and V1 is the volume of HNO3 and M2 is the molarity and V2 is the volume of…
Q: The equivalence point is reached when a solution is neutralized. OTrue O False
A: This question can be solved by considering the case of acid-base titration, in which a definite…
Q: What is the concentration of a household ammonia cleaning solution if 49.90 mL of 0.5900M HCl is…
A: The balanced chemical equation is, HCl+NH3→NH4++Cl- The number of moles=(Molarity)(Volume of…
Q: 15.0 mL of unknown HCI solution was titrated by 0.15 M of NaOH. 37.78 mL of that NaOH solution was…
A: The neutralisation reaction taking place is NaOH + HCl ------> NaCl + H2O
Q: By titration, it is found that 77.3 mL of 0.122 M NaOH(aq) is needed to neutralize 25.0 mL of…
A: Answer: In neutralization reaction, hydroxide ion of base reacts with hydrogen ion of acid and…
Q: By titration, it is found that 13.5 mL of 0.112 M NaOH(aq) is needed to neutralize 25.0 mL of…
A: Since the reaction taking place is given by NaOH + HCl ----> NaCl + H2O Hence we can say that 1…
Q: What volume (in mL) of 0.2800 M HBr is required to neutralize 50.00 mL of 0.7000M KOH?
A: For a balanced chemical reaction.aA+bB→cC+dDMoles of A reacteda=Moles of B reactedb=Moles of C…
Q: A 0.261 g sample of NaHC204 (one acidic proton) required 17.5 mL of sodium hydroxide solution for…
A: To calculate the concentration of NaOH, we need to determine the moles of NaHC2O4. As we know number…
Q: Suppose 26.0 mL of 0.100 M HCl(aq) were spent to completely neutralize 10.0 mL of an ethylamine…
A: Hydrochloric acid reacts with amine to form ammonium chloride.
Q: What volume (in mL) of 0.2800 M HBr is required to neutralize 50.00 mL of 0.7000 M KOH?
A: Mixing of water is called dilution Voulme is =125ml
Q: What volume (in mL) of 0.2600 M HBr is required to neutralize 50.00 mL of 0.7000 M KOH?
A: Let the volume of HBr = V1 Molarity of HBr=…
Q: What volume (in mL) of 0.2850 M HBr is required to neutralize 50.00 mL of 0.7000 M KOH?
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Q: What volume (in mL) of 0.3000 M HBr is required to neutralize 60.00 mL of 0.6000 M LiOH?
A: Given , Molarity of HBr , M1 = 0.3000 M Molarity of LiOH , M2= 0.6000 M V2= 60.00 ml
Q: If it requires 17.86 mL of a 0.278 M NaOH solution to titrate a 25.00 mL HCl solution, what is the…
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Q: What is the molarity of an HCl solution if 42.8 mL of it is titrated to the equivalence point with…
A: Given information: [NaOH] = 1.07 M Volume for NaOH = 20.1 mL Volume for HCl = 42.8 mL
Q: A 15.0 mL solution of Ba(OH)2 is neutralized with 34.4 mL of 0.200 M HCI. What is the concentration…
A: Given, Molarity of HCl = 0.200 M Volume of HCl = 34.4 ml Volume of solution = 15.0 ml The chemical…
Q: By titration, it is found that 55.5 mL of 0.116 M NaOH(aq) is needed to neutralize 25.0 mL of…
A: HCl(aq) + NaOH (aq) ------> NaCl (aq) + H2O (l) Number of moles of HCl = Number of…
Q: A 0.110 L sample of an unknown HNO3 solution required 48.5 mL of 0.100 M Ba(OH)2 for complete…
A: According to the given question, the HNO3 solution is titrated with Ba(OH)2.For this acid-base…
Q: What volume (in mL) of 0.2050 M HCI is required to neutralize 50.00 mL of 0.8000 M NaOH?
A: HCl + NaOH --> NaCl + H2O at complete neutralization moles of acid =…
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: By titration, it is found that 70.1 mL of 0.161 M NaOH(aq) is needed to neutralize 25.0 mL of…
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Q: What volume, in ml, of 0.5000M HCN can be made from 16.28ml of 14.37M HCN?
A: Given that: V1 = 16.28 ml and S1 = 14.37 M V2 = ? and S2 = 0.5 M
Q: What volume (in mL) of 0.2300 M HBr is required to neutralize 50.00 mL of 0.7000 M KOH?
A: The reaction of an acid and base to produce salt and water is called as neutralization reaction. For…
Q: By titration, it is found that 63.5 mL of 0.104 M NaOH(aq) is needed to neutralize 25.0 mL of…
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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: By titration, it is found that 39.1 mL of 0.161 M NaOH(aq) is needed to neutralize 25.0 mL of…
A: Balanced chemical equation: NaOH + HCl -----> NaCl + H2O Number of mmoles of NaOH = Number…
Q: A 45.0 mL solution of LiOH is neutralized with 36.5 mL of 0.350 M HCl. What is the concentration of…
A: Given The volume and concentration of HCl and the volume of LiOH. To find Concentration of LiOH in…
Q: In an experiment, 20.11 mL of 0.102 M LIOH is required to complete neutralize a 12.36 mL of…
A: To solve this problem we first calculate the number of mile of LiOH from its molarity and volume…
Q: If 8.00 mL of a hydrochloric acid solution had a known concentration of 0.3456 M, how many mL of a…
A: Given: The volume of hydrochloric acid (HCl) is 8.00 mL The concentration of hydrochloric acid is…
Q: concentration
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Q: A 15.0 mL solution of Ba(OH)₂ is neutralized with 21.4 mL of 0.200 M HCl. What is the concentration…
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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: Suppose that 250.0 mL of a basic solution is 0.100 M in KOH. What volume of a 0.200-M HCl solution…
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Q: A 15.0 mL solution of Ba(OH)2 is neutralized with 34.6 mL of 0.200 M HCI. What is the concentration…
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Q: A 20.0 mL solution of NaOH is neutralized with 23.0 mL of 0.200 M HBr. What is the concentration of…
A: Step 1 Given Data Sodium Hydroxide Volume = 20 mL (V2) HBr Solution Volume = 23 mL (V1) HBr…
Q: A 45.0-mL sample of a 0.837 M HNO, solution is titrated with a 0.338 M KOH solution. What will be…
A: In this titration reaction, HNO3 is a strong acid and KOH is a strong base. HNO3 is exactly…
Q: A 15.0 mL solution of Ba(OH)2 is neutralized with 34.8 mL of 0.200 M HCI. What is the concentration…
A: The neutralisation reaction taking place can be written as, => HCl + Ba(OH)2 ----------> BaCl2…
Q: What volume (in mL) of 0.2650 M HCl is required to neutralize 50.00 mL of 0.8000 M NaOH?
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Q: In a titration, 25.0 mL of NaOH is completely neutralized by 15.0 mL of 0.500 M HCl. What is the…
A: We should know the balanced reaction for titration for predicting equivalence point. We have given…
Q: A solution of hydrochloric acid has a volume of 280. mL and a pH of 1.92. Exactly 160. mL of 0.0100…
A: Solution stoichiometry involves the calculation of concentration of solutions in the given…
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- An unknown mixture is known to contain only Ba(OH)2 (MW=171.34 g/mole) and NaOH (MW=40.0 g/mole). If the mixture is known to contain 45% by mass NaOH, and 8.0 grams of the mixture is dissolved completely in 50.0 ml of solution, answer the following. a). How many ml of 0.2 M H2SO4 is needed to titrate the 50.0 ml solution to the equivalence point.What weight of sample should be taken for analysis sos that the volume of 0.1074N NaOH used for titration equals the percentage of potassium acid phthalate (KHC8H4O4) in the sample (Answer 2,193 g)Solve correctly please. A 100 mL solution is prepared by weighing 1.50 g from the mixture of KI and KBr. When the 20 mL part taken from this solution is titrated with 0.02 M AgNO3 solution, 105 mL is consumed. Accordingly, calculate the percentage of Kl in the mixture. (KI: 166 KBr: 119 g/mol) A. 56.3 B. 59 C. 41 D. 43.7 (Gpt/ai wrong answer not allowed)
- A mixture containing KCl and NaBr was analyzed by Mohr's method. A mass of 0.31011 g of the mixture was dissolved in 50 mL of water, the Na2CrO4 indicator was added, and it was titrated with a 0.11011 mol/L AgNO3 solution. The endpoint was 36.011 mL. What are the % m/m concentrations of KCl and NaBr in the mixture?1. Calculate the moles of KHP you titrated for each trial. (KHP is KHC8H4O4). MW = 204.23 g/mol. Determine the number of moles of NaOH required to neutralizw the KHP. Use the mole-mole ratio provided inthe balanced equation. Place answers in data table 2(second picture format) 2. Calculate the volume, in mililiters, of NaOH used to neutralize the KHP. Convert to Liters. Place answers in data table 2. 3. Calculate the molarity of the NaOH solution in units of moles/liter. Place answers in data table 2.a) How many mL of concentrated HCl solution are needed to prepare 250 mL of a 0.36 M HCl solution? Concentrated HCl solution is 35.0% HCl by weight and has a density of 1.19 g/mL. (H: 1, Cl: 35.5 g/mol) b) To standardization of this hydrochloric acid solution, 0.2548 g of sodium carbonate requires 14.0 mL of HCl solution for titration to the equivalence point with methyl orange as indicator. What is the molarity of the HCl solution? (H:1, O:16, Cl: 35.5, Na: 23, C: 12 g/mol)
- It required 11.96 mL of 0.102 M NaOH to titrate a 0.0927 g sample of an unknown monoprotic acid to the endpoint using phenolphthalein as an indicator. What is the molar mass of the unknown acid?A saturated solution of strontium hydroxide is repaired in the excess solid Sr(OH)2 is allowed to settle. A 25ml aliquot of the saturated solution is withdrawn and transferred to a flask, and two drops of indicator. A 0.073 M HCl solution is used to titrate the hydroxide ion, requiring 29.50 ml to reach the end point. What is the molar concentration of the hydroxide ion in the saturated solution?Maleic acid (H2C4H2O4, represented by H2M) is the precursor of malic acid widely used in industry. food as an acidulant and in the pharmaceutical industry it is used in the treatment of wounds. This acid can be determined by neutralization titration. Answer the items below about this determination. Considering a 15.0 mL sample of maleic acid-based product used in industry, determine the maleic acid concentration, in mol/L, in the sample knowing that 21.7 mL of a solution of 0.1120 mol/L NaOH for complete neutralization of this acid. How many grams of maleic acid were in the sample analyzed and what is its percentage (%, m/v) in the sample? [Answer; m=0.1405 mol L-1; percentage = 0.9365%] NaOH(aq) + H2M(aq) Na2M (aq) + H2O(l) Suggest an appropriate indicator for the titration of this acid by looking at the titration curve profile below (IMAGE)
- 17.5 milliliters of a 0.496 M RbOH solution are required to titrate 52.1 milliliters of a H3PO4 solution. What is the molarity of the H3PO4 solution?3RbOH + H3PO4 --> Rb3PO4 + 3H2O Please put answer in box with 3 digits past decimal in regular non scientific notation.You are performing an experiment in lab that involves the titration of 25.0 mL of H2SO4 solution. You titrate the acidic solution with 0.8067 M NaOH and the equivalence point is reached by the addition of 17.31 mL of NaOH solution. Using the balanced equation below, calculate the molartity of H2SO4 in the flask. Do NOT include units. 2NaOH(aq) + H2SO4(aq) --> 2H2O(l) + Na2SO4(aq)100.0 mL of a 0.245 M solution of HCl was added to 50.0 mL of 0.365 M Ba(OH)2. Answer the following. a. Identify the limiting and excess reagents. b. How much more (volume in mL) of the limiting reagent is needed to titrate to the equivalence point? c. What mass of BaCl2 could be obtained if the solution was dried?