Home
Class 11
CHEMISTRY
How would you make up 425 mL of 0.150M H...

How would you make up 425 mL of 0.150M `HNO_3` from 68.0% `HNO_3`? The density of 68.0% `HNO_3` is1.41g/mL.

Text Solution

Verified by Experts

The correct Answer is:
`4.25`
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL CALCULATION

    NCERT GUJARATI|Exercise Question ( Choose the best answer :)|17 Videos

  • CHEMICAL CALCULATION

    NCERT GUJARATI|Exercise Question ( Fill in the blanks )|7 Videos

  • CHEMICAL CALCULATION

    NCERT GUJARATI|Exercise EXAMPLE|3 Videos

  • CHEMICAL BONDING

    NCERT GUJARATI|Exercise Questions(E. Explain briefly on the following)|1 Videos

  • CHEMICAL EQUILIBRIUM - I

    NCERT GUJARATI|Exercise Questions(E. Explain briefly on the following)|2 Videos

Similar Questions

Explore conceptually related problems

What volume of 0.250 M HNO_3 reacts with 42.4 mL of 0.150 M Na_2CO_3 in the following reaction ? 2HNO_(3(aq)) + Na_2 CO_(3(aq)) -> 2NaNO_(3(aq)) + H_2O_((aq)) + CO_(2(aq))

A disposable galvanic cell Zn|Zn^(2+)||Sn^(2+)|Sn is produced using 1.0 mL of 0.5 M Zn(NO_(3))_(2) and 1.0 mL of 0.50 M Sn(NO_(3))_(2) . It is needed to power a pace maker that draws a constant current of 10^(-6) Amp to run it and requires atleast 0.50 V to function. Calculate the value of |Zn^(+2)| when cell reaches 0.5V at 298K . (Given: E^(@) (Zn^(2+)//Zn) =- 0.76V: E^(@) (SN^(2+)//Sn) =- 0.14V) .

Nitric acid, HNO_3 is a colourless, corrosive liquid used in the manufacture of Nitrogen fertilizers and explosives. In an experiment to develop new explosives for mining operations, a 28.5 g sample of HNO_3 was poured into a beaker. How many moles of HNO_3 are there in this sample of HNO_3 ?

NCERT GUJARATI-CHEMICAL CALCULATION -Problems of Practice
  1. A compound contains 32% carbon, 4% hydrogen and rest oxygen. Its vapou...

    Text Solution

    |

  2. An acid of molecular mass 104 contains 34.6% carbon, 3.85% hydrogen an...

    Text Solution

    |

  3. What is the simplest formula of the compound which has the following p...

    Text Solution

    |

  4. Calculate the oxidation number of underlined elements in the following...

    Text Solution

    |

  5. Calculate the oxidation number of underlined elements in the following...

    Text Solution

    |

  6. Calculate the oxidation number of underlined elements in the following...

    Text Solution

    |

  7. Calculate the oxidation number of underlined elements in the following...

    Text Solution

    |

  8. Calculate the oxidation number of underlined elements in the following...

    Text Solution

    |

  9. Balance the equations Mg + NO3^(-) to Mg^(2+) + N2O + H2O) ( in acidi...

    Text Solution

    |

  10. Balance the equations Cr^(3+) + Na2O2 to CrO4^(-) + Na^(+)

    Text Solution

    |

  11. Balance the equation S^(2-) + NO3^(-) to NO + S8

    Text Solution

    |

  12. Balance the equations FeS + O2 to Fe2O3 + SO2 ( molecular form )

    Text Solution

    |

  13. Balance the equations Cl2 + OH^(-) to Cl^(-) + ClO3^(-) + H2O

    Text Solution

    |

  14. Calculate the volume of 14.3 M NH3, solution needed to prepare 1L of 0...

    Text Solution

    |

  15. How would you make up 425 mL of 0.150M HNO3 from 68.0% HNO3? The densi...

    Text Solution

    |

  16. Calculate the molarity of a solution obtained by mixing 100 mL of 0.3 ...

    Text Solution

    |

  17. Calculate the molality of a solution by dissolving 0.850g of ammonia (...

    Text Solution

    |

  18. NiSO4 reacts with Na3PO4 to give a yellow green precipitate of Ni3 (PO...

    Text Solution

    |

  19. What volume of 0.250 M HNO3 reacts with 42.4 mL of 0.150 M Na2CO3 in t...

    Text Solution

    |

  20. A flask contains 53.1 mL of 0.0150 M Ca(OH)2 solution. How many mL of ...

    Text Solution

    |